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chem exam 2
| Question | Answer |
|---|---|
| The electron from a hydrogen atom drops from an______ state into the_______ state. When an electron drops into a lower-energy orbital, energy is released in the form of ________ _________ | excited; ground; electromagnetic radiation |
| How much energy does the electron have initially in the n=4 excited state? | -1.37 x 10^-19 J |
| What is the change in energy if the electron from Part A now drops to the ground state? | -2.05 x 10^-18 J |
| What is the wavelength λ of the photon that has been released in Part B? | 9.70 x 10^-8 m |
| What might the photon from Part C be useful for? | getting a suntan |
| Just as light waves have________ behavior, a moving particle has a_______ nature. | particle; wave |
| The faster the particle is moving, the________ its kinetic energy and the_______ its wavelength | higher; shorter |
| The mass of an electron is 9.11×10−31 kg. If the de Broglie wavelength for an electron in a hydrogen atom is 3.31×10−10 m, how fast is the electron moving relative to the speed of light? The speed of light is 3.00×108 m/s. | .732% |
| The mass of a golf ball is 45.9 g . If it leaves the tee with a speed of 80.0 m/s , what is its corresponding wavelength? | 1.80 x 10^-34 |
| Every electron in an atom has a_________ set of four quantum numbers. | unique |
| The ________________corresponds to the shell in which the electron is located. Thus n can therefore be any integer. | principal quantum number n |
| an electron in the 2p subshell has a principal quantum number of ________because 2p is in the second shell. | n=2 |
| The ______________corresponds to the subshell in which the electron is located. can have integer values ranging from 0 to n−1. | angular momentum quantum number ℓ |
| for angular momentum quantum number, s subshells are coded as ___, p subshells as __, d as ___, and f as ____. | 0; 1; 2; 3 |
| The _________________ corresponds to the orbital in which the electron is located | magnetic quantum number mℓ |
| As a rule, mℓ can have integer values ranging from _____________ | −ℓ to +ℓ. |
| The ____________ corresponds to the spin of the electron in the orbital. A value of 1/2 means an "up" spin, whereas −1/2 means a "down" spin. | spin quantum number ms |
| What is the only possible value of mℓ for an electron in an s orbital? | 0 |
| What are the possible values of mℓ for an electron in a d orbital? | -2, -1, 0, 1, 2 |
| PART C #9 CH 3 HW | |
| The three dimensional plot represents the area where electrons are most likely to be found in each orbital. Where the distribution has a_____, such as at the center of the p orbital where the two lobes meet, the probability of finding an electron is_____. | node; zero |
| The probability of finding an electron at a point in an atom is referred to as the ________ __________ | probability density |
| The 4f orbitals have_______ nodes.The 3p orbitals have______ nodes. | three; two |
| In general, the number of radial nodes = ___-____-_____ | (n−ℓ)−1. |
| PROBLEM 11 CH 3 HW | |
| when n= these numbers what does l=? n= 1, 2, 3, 4 | l = 0 0,1 0,1,2 0,1,2,3 |
| PROBLEM 13, 14 CH 3 HW | |
| The minimum energy required to change the conformation of 11-cis-retinal within the eye is about 164 kJ/mol. Calculate the longest wavelength visible to the human eye. | ??? |
| know difference between main group elements, transition metals, and inner transition metals | |
| ________ are the horizontal row on the periodic table | periods |
| where are the mtals on the periodic table? | to the left of staircase except hydrogen |
| where are the nonmetals on the periodic table? | to the right of the staircase |
| what are the metalloids? | boron, silocon, Ge, As, Sb, Te, Po |
| The elements from group 3 to group 12 in the periodic table are often called the________ _________. These elements exhibit the characteristic properties of this and are often found in more than one _________state. | transition metals; one oxidation |
| In the group 3 to group 12 elements, which subshell is filled up going across the rows? | d subshell |
| In period 4 of the table, the ____subshell fills, and in periods 5 and 6, the ____ and _____subshells fill, respectively. | 3d ; 4d and 5d |
| A sample of soil from a newly discovered cave. They find an element that is a good conductor of electricity. It also forms a chloride in the form XCl2 and an oxide in the form XO. The element is a liquid at room temperature. | Hg |
| Give the complete ground-state electron configuration for silicon (Si). | 1s^2 2s^2 2p^6 3s^2 3p^2 |
| Give the ground-state electron configuration for silicon (Si) using noble-gas shorthand. | [Ne] 3s^2 3p^2 |
| Give the actual ground-state electron configuration for copper (Cu) using the complete form. | 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^10 |
| Give the ground-state electron configuration for copper (Cu) using noble-gas shorthand. | [Ar]4s^1 3d^10 |
| The periodic table lists all known elements arranged by ______ ______. Atomic number is the______ charge, the number of________ in the nucleus of an an atom of a particular element. | atomic number; nuclear; protons |
| Each column of the table, called a________, contains elements with the same number of _______ ________ that are in different_________ levels. | group; valence electrons; quantum |
| Each row of the table, called a________, contains elements with differing numbers of ______ ________ that are in the same _______ _______ level. | period; valence electrons; principal quantum; |
| The four main blocks of the table (_,__,_,_)) contain elements whose highest energy electrons have the same ______ ________ | (s, p, d, and f; azimuthal quantum number (ℓ). |
| The ______________of an element includes everything except the noble-gas core. For example, the element C has an electron configuration of [He]2s22p2 and an outer electron configuration of what? | outer electron configuration ; 2s^2 2p^2 |
| ch 4 homework number 4 | |
| principle that states Electrons are added to the lowest energy orbitals available. | aufbau |
| principle that states No two electrons in an atom can have the same set of four quantum numbers (n, ℓ, mℓ, and ms). | pauli exclusion principle |
| so for a degenerate set of orbitals, one electron goes into each orbital until all the orbitals of the subshell are half-filled. Once all the orbitals of the subshell are half-filled the pairing of electrons can take place. | hund's rule |
| part b question 5 chapter 4 hw | |
| Quantum numbers are used to uniquely identify an_______ in an atom. The _______ _________principle states that no two electrons in an atom may have the same set of four quantum numbers. | electron; Pauli exclusion |
| List a possible set of four quantum numbers (n, ℓ, mℓ, ms) in order, for the highest energy electron in gallium, Ga. | 4, 1, -1, 1/2 |
| An _____________ diagram shows the number of electrons in each orbital, which are shown in order of energy. | orbital-filling |
| 3 main rules in orbital-filling diagrams | 1. lower energy subshells fill before higher energy 2. an orbital can hold up to 2 electrions, which must have opposite spins 3. hund's rule aka bus rule |
| How many orbitals are there in the third shell (n=3)? | 9 - (one s, three p, and five d) |
| Show the orbital-filling diagram for N (nitrogen). S | answer # 7 ch 4 |
| Show the orbital-filling diagram for S (sulfur). | answer # 7 ch 4 |
| Show the orbital-filling diagram for Br (bromine). | answer # 7 ch 4 |
| # 8 chapter 4 | |
| Name an element in the third period (row) of the periodic table with three valence electrons. | Al |
| Name an element in the third period (row) of the periodic table with four 3p electrons. | S |
| Name an element in the third period (row) of the periodic table with six 3p electrons. | Ar |
| Name an element in the third period (row) of the periodic table with two 3s electrons and no 3p electrons. | Mg |
| Determine the number of valence electrons - Ga | 3 |
| Determine the number of valence electrons - Sn | 4 |
| Determine the number of valence electrons - Br | 7 |
| Determine the number of valence electrons - Se | 6 |
| Which elements do you expect to lose electrons in their chemical reactions? Which do you expect to gain electrons? Ga, Sn, Br, Se | lose - Ga, Sn gain - Br, Se |
| Elements with ____ or fewer valence electrons tend to lose electrons, and elements with ____or more valence electrons tend to gain electrons | 3; 5 |
| A positive ion is called a_______ whereas a negative ion is called an______. | cation; anion |
| What is the charge on the most stable ion of each of the following elements? K, Ba, Mg, Al, N, O, S, I (range from 1+ to 1-) | 1+ - K, 2+=Ba, Mg; 3+=Al 3-:N; 2- = O, S; 1 - =I |
| A main group_____ tends to lose electrons, forming a cation with the same number of electrons as the nearest noble gas in the periodic table. | metal |
| A main group________ tends to gain electrons, forming an anion with the same number of electrons as the nearest noble gas. | nonmetal; |
| If the following elements were to form ions, they would attain the same number of electrons as which noble gas? Be, N, Mg, K, P, Se, Sr | Be = He N, Mg = Ne K, P = Ar Se, Sr = Kr |
| A certain element forms an ion with 18 electrons and a charge of +2. Identify the element. | Ca |
| The ______ _________ of an atom tells us how many electrons are in each orbital. | electron configuration |
| What is the ground-state electron configuration of a neutral atom of manganese? | [Ar]4s^2 3d^5 |
| What is the ground-state electron configuration of the chloride ion Cl−? | [Ne]3s^2 3p^6 |
| Which element has the following configuration: [Xe]6s24f5? | Pm |
| Main group metals lose electrons in the_______ order of filling. Transition metals, however, lose___ _________ first. | reverse; s electrons |
| In the ground-state electron configuration of Fe3+, how many unpaired electrons are present? | 5 |
| Build the orbital diagram for the ion most likely formed by phosphorus. | answer ch 4 hw #14 |
| Each element in the periodic table has a distinctive atomic________. | radius |
| Place the following elements in order of decreasing atomic size: antimony, selenium, fluorine, rubidium, strontium, and arsenic. | Rubidium, Strontium, Antimony, Arsenic, Selenium, Flurine |
| what does ionic radii mean | The more electrons that are lost, the smaller the ion becomes. more electrons gained, larger the ion becomes |
| Rank the following ions in order of decreasing radius: F−,Cl−,Br−,I−, and At−. | At-, I-, Br-, Cl-, F- |
| Rank the following items in order of decreasing radius: Ca, Ca2+, and Ca2− | Ca2-, Ca, Ca2+ |
| In a group of ions with the same number of electrons, the most________ ion is the largest and the most________ ion is the smallest. | negative; positive - part C ch 4 hw # 16 |
| Predict the charge of the ion formed by each of the following elements. Ca | Ca 2+ |
| Predict the charge of the ion formed by each of the following elements. Cl | Cl - |
| Predict the charge of the ion formed by each of the following elements. F | F - |
| Predict the charge of the ion formed by each of the following elements. Na | Na + |
| Arrange the following elements in order of decreasing atomic radius: Ba, Sb, Cl, Tl, and As. | Ba, Tl, Sb, As, Cl |
| As you move down a column (or family) in the periodic table, atomic radius________. As you move to the right across a period (or row) in the periodic table, atomic radius___________. | increases; decreases |
| draw electron configurations for Cl-, P 3- , K+, Mo 3+ , V 3+ | answers #19 ch 4 hw |
| Write orbital diagram for: Cd2+, Au+., Mo3+., Zr2+..and determine if its diamagnetic or paramagnetic | answers #20 ch 4 hw |
| Arrange the following isoelectronic series in order of increasing atomic radius: Cl−, Sc3+, S2−, Ca2+, and K+. | Sc3+ Ca2+ K+ Cl− S2− |
| the number of_________ affects the radii of an ion even as the number of electrons remains constant. | protons |
| who invented the quantum mechanical model of the atom | Neils Bohr |
| what are Bohr's 3 postulates? | only orbits of a certain radii are allowed, an electron in an allowed orbit has a specific energy, energy is absorbed or emitted only when the electron moves from one allowed orbit to another |
| n = | principle quantum number |
| B = | 2.18 x 10^-18 J |
| Why does an electron orbit nuclei in an atom? What force? | electromagnetism - negative electron charge attracts the positive proton charge; energy has force associated with it |
| As n grows, or the electron moves away from the center of the atom, energy ___________ | increases |
| what is your change in energy going to be like if your final n is greater than your initial n and what does that mean in terms of photons? | change in energy will be positive and that means you absorbed a photon |
| what is your change in energy going to be like if your final n is less than your initial n and what does that mean in terms of photons? | change in energy will be negative and you will emit a photon |
| the charge of delta E tells you what? | which direction energy is flowing |
| the change in energy is equal to the energy of a __________ | photon |
| if an electron with an initial n of 3 jumps to a n final of 1, what color is the photon? absorbed or emitted? | UV, emitted delta E = -1.94 x 10^-18 J WAVELENGTH = -102.46 nm |
| when finding wavelength, you have to use the ________ value of energy | absolute |
| the lines in the line spectrum represent what? | specific orbital transition |
| what is the analogy of chemistry postal addressing | n = state l = city m sub l = street spin or m sub s = house # |
| as n increases, size __________ | increases - orbital gets bigger |
| as n increases, energy __________ | increases - size is increasing, farther away from nucleus, attraction is less, energy goes up |
| what are the integer values for n | positive integers starting with 1 |
| what are the integeer values for l | 0 - (n-1) |
| what are the l values for the orbitals | 0=s 1=p 2=d 3=f |
| integer values for magnetic quatum # | -L to L aka # of orbitals |
| values for spin quantum number | +1/2, -1/2 |
| LOOK AT SHAPES OF ORBITALS IN NOTES | |
| how electrons occupy orbitals | electron configuration |
| when all electrons are in their lowest energy orbitals | ground state |
| electrons are in higher orbitals | excited state |
| when you go from ground to excited state, you ___________ a photon | absorb |
| when you go from excited to ground state you________ a photon | emit |
| the rule that states that it takes 8 electrons to be stable | octet rule |
| fluorine is an ________ because it wants to take an electron from something else; Fl^-1 is very stable, fluorine is very reactive | oxidant |
| what are some main characteristics of metals | metals - good conductors of heat and electricity, tends to be shiny, malleable, ductile |
| what are some characteristics of nonmetals | insulator of electicity and heat, tend to be dull, a lot are gases |
| since metal atoms are able to rearrang themselves, the are very ________ and _________ | ductile |
| nonmetals are very ________ so if you pound them they will shatter | brittle |
| metalloid characteristics | semi conductors |
| group 1, 2, 5, 6, 7, 8 names | 1 - alkali metals 2 - alkaline earth metals 5 - nictides 6 - calcogens 7- halogens 8-noble gases |
| when electron clouds start to comingle, ____________ force repels them away. boundary in atomic size is due to comingling of the ________ __________ | electrostatic force; electron clouds |
| as you go down and to the left, atomic radius __________ | increases |
| what group is the largest atoms | alkali metals |
| at least one unpaired spin | paramagnetic |
| what is the consequence of being paramagnetic | aligns and interacts with the magnetic field |
| no unpaired spins | diamagnetic |
| consequence of being diamagnetic | do not align in the magnetic field and somewhat repels magnetic fields |
| something can be twice as paramagnetic as something else | just know |
| whats a give away that something is going to be paramagnetic | if it has an odd number of electrons |
| _________ are smaller than parent atoms while __________ are larger than parent atoms | cations; anions |
| isoelectronic rule - what do iso and electronic mean | iso - same electronic - electron configuration |
| what does the isoelectronic rule mean | if they have the same electron configuration, the way you tell is by the amount of protons - smaller have more protons and olarger have less |
| ionization energy __________ as you go up because you have fewer electrons | increases |
| ____________ ____________is the amount of energy required to remove an electron from a neutral gaseous atom or gaseous ion. | Ionization energy (Ei) |
| Electrons are attracted to the positively charged nucleus; therefore removing an electron requires_________ | energy |
| The process of ionization energy is________, and so ionization energies have a________ value | endothermic; positive |
| The______ ionization energy (Ei1) is the energy associated with the removal of an electron from the neutral gaseous atom. | first |
| reaction equation for first ionization energy for generalized atom X | X→X+ + e− |
| The amount of energy required to remove an electron is related to the effective________ charge and the_______ of the electron configuration of the atom. | nuclear; stability |
| ionization energy shows periodic variation generally increasing from______ to________ in a period and from bottom to top of a group | left; right |
| Removal of successive electrons always requires_______ energy (e.g., Ei3>Ei2>Ei1) because a negative electron is being removed for a successively higher positive charge | more |
| An important property that results from the electron configuration of an atom or an ion is behavior in the presence of an external ______ _________ | magnetic field. |
| Due to the random orientations of electron________ most materials have no permanent magnetic effect without an external magnetic field. | spins |
| The magnetic behavior of an atom or ion depends on its _______ ___________. | electron configuration |
| The origin of magnetism lies in the_______ and_______ motions of electrons and how the electrons interact with one another. | orbital; spin |
| Each electron in an atom moving about the nucleus while spinning about its own axis gives rise to an________ field and a consequent_________ field. | electric; magnetic |
| A _______ _________is assigned to each electron to describe the magnetic field produced. | magnetic moment |
| The total magnetic moment of the substance is the vector sum of individual ________ ___________ of individual electrons. | magnetic moments |
| If two electrons are oriented in the opposite direction, their vectors are in equal in magnitude but opposite direction; therefore their vector sum will be _______ | zero |
| Application of an external magnetic field, unpaired electron spins causes the orientation of unpaired electron spins to become aligned with the external field. alignment causes a change in the magnetic moment results in attraction to the external field. | These substances are termed paramagnetic. |
| application of an external magnetic field to a substance whose electron spins are all paired causes a change in the magnetic moment that results in a magnetic field that is in opposition to the external field and a slight repulsion to the external field. | These substances are termed diamagnetic. |
| In a________ atom or ion, all electrons are paired, and the individual magnetic effects cancel out. species is weakly repelled by an external magnetic field. | diamagnetic |
| A__________ atom or ion has unpaired electrons, and the individual magnetic effects do not cancel out. Each unpaired electron possesses a magnetic moment that causes the atom or ion to be attracted to an external magnetic field. | paramagnetic |
| _____________, is the change in energy that occurs when an electron is added to a neutral isolated atom. | Electron affinity, Eea |
| equation for electron affinity | X(g)+e−→X−(g) |
| Most electron affinity values are_________ because energy is usually released when a neutral atom gains an electron. | negative |
| Eea values become more__________ with increasing tendency of the atom to_________ an electron and increasing_________ of the resulting anion. | negative; accept; stability |
| Elements with________ than an octet and with high effective nuclear charge (Zeff) tend to have_______ negative Eea values. Elements with filled valence shells or subshells and low Zeff tend to have Eea values near_______. | less; large; zero |
| Consider the following neutral electron configurations in which n has a constant value. Which configuration would belong to the element with the most negative electron affinity, Eea? 3s 2 3s2 3p2 3s2 3p5 3s2 3p6 | 3s2 3p5 |
| part B chapte 4 #24 | |
| A covalent bond occurs when atoms share electrons. The resulting cluster of atoms is called a molecule, and the compound is considered to be___________. | molecular |
| For the elements with the electron affinities given in the table in the introduction, which element is most likely to accept an electron? Ca, S, N | S |
| Rank the following elements by electron affinity, from most positive to most negative EA value. potassium, arsenic, helium, bromine, sulfur | helium, potassium, arsenic, sulfur, bromine |
| The reason why group 8A elements have a________ EA value is because they are incredibly stable in their neutral form with an octet of electrons in the outermost energy level. | positive |
| The reason that group 5A elements have an EA value that is less________ than expected is because a half-filled p subshell is particularly stable. | negative |
| Arrange the following elements in order of decreasing first ionization energy: Bi, Cl, Te, and S. | Cl, S, Te, Bi |
| A________ bond occurs when atoms share electrons. The resulting cluster of atoms is called a molecule, and the compound is considered to be_________. | covalent; molecular |
| An________ bond results from a transfer of one or more electrons from one atom to another. This creates oppositely charged ions that group together into large macroscopic lattices as opposed to small clusters. | ionic; |
| As a general rule,________ bonds occur between two nonmetal atoms whereas________ bonds occur between a metal and a nonmetal atom. | covalent; ionic |
| When main group elements react, they tend to acquire eight outer-shell electrons (ns2np6). This is called an_______, and it is a particularly stable configuration. | octet |
| _______in the________ period and beyond can break the octet rule because they have vacant d orbitals that allow them to accommodate more than eight outer-shell electrons. | Nonmetals; third |
| An unknown element, X, reacts with rubidium to form the compound Rb2X. In other compounds this element also can accommodate up to 12 electrons rather than the usual octet. What element could X be? | S |
| Predict the product(s) of the following reaction: Cs + Br2 ⇌ | CsBr |
| Predict the products of the following reaction: Rb + N2⇌ | no reaction - only lithium is small enough to react with nitrogen of all the alkali metals |
| #5 , #6 chapter 5 | |
| compound between Li and N | Li3N |
| compound between Al and Br | AlBr3 |
| compound bt Al and S | Al2S3 |
| compound bt Ba and F | BaF2 |
| _________names are historical and tend not to identify the elements that make up the compound. | Common |
| the__________ name allows for correct identification of the cations and anions that together make up the ionic compound. | systematic |
| What is the chemical formula for potassium permanganate? | KMnO4 |
| Blue vitriol is commonly used in industrial dyeing processes. What is the chemical formula for blue vitriol, whose systematic name is copper(II) sulfate? | CuSO4 |
| Sodium carbonate is used in the manufacture of paper. What is the chemical formula for this compound? | Na2CO3 |
| Binary ionic compounds are named by identifying first the________ ion and then the________ ion. Naming compounds with_________ ions involves memorizing the names and formulas of the most common ones. | positive; negative; polyatomic |
| Give the systematic name for the compound Al(NO3)3. | aluminum nitrate |
| Only those metals with more than one________ state must have its state written in the name. | oxidation |
| Give the systematic name for the compound Mn2(SO4)3. | manganese (III) sulfate |
| Enter the formula for the compound calcium oxide. | CaO |
| Enter the formula for the compound copper(II) phosphate. | Cu3(PO4)2 |
| What is the systematic name of Mg(NO3)2? | magnesium nitrate |
| What is the systematic name of NH4ClO3? | ammonium chlorate |
| What is the systematic name of PbO? | lead (II) oxide |
| rubidium and carbonate formula | Rb2CO3 |
| rubidium and phosphate formula | Rb3PO4 |
| rubidium and hydrogen phosphate formula | Rb2HPO4 |
| rubidium and acetate formula | CH3CO2Rb |
| lead (II) chloride formula | PbCl2 |
| copper (I) iodate formula | CuIO3 |
| Potassium chromate formula | K2CrO4 |
| copper (I) fluoride formula | CuF |
| iron (III) hydroxide formula | Fe(OH)3 |
| irion (III) phosphate formula | FePO4 |
| LOOK AT POLYATOMIC IONS AND MEMORIZE THEM | |
| How many covalent bonds does carbon form in neutral compounds? | 4 |
| How many covalent bonds does oxygen form in electrically neutral compounds? | 2 |
| How many covalent bonds does nitrogen form in electrically neutral compounds? | 3 |
| How many covalent bonds does hydrogen form in electrically neutral compounds? | 1 |
| In a covalent bond between two atoms, the more electronegative atom will attract more electron density toward itself, causing a_______ bond. | polar |
| The magnitude of the bond polarity is the_________ in electronegativity values of the atoms | difference |
| In the molecule FBr, which atom is the negative pole? | F |
| Of the molecules SiCl4 and SiI4, which has bonds that are more polar? | SiCl4 |
| All three of the phosphorus-fluorine single bonds in PF3 are polar. In which direction should the polarity arrows point? | away from the central phosphorus atom |
| Electronegativity is a value that is determined for each element according to its _____ _______ and its _______ ________ | electron affinity; ionization energy. |
| the most electronegative element,_________, at 4.0. | fluorine |
| Note that electronegativity values tend to________ going across the rows of the periodic table and to_________ going down the columns of the periodic table. | increase; decrease |
| The strongly electronegative elements, found in the upper right corner of the periodic table, have a tendency to gain electrons in chemical reactions and are therefore good_________. | oxidizers |
| The weakly electronegative elements, making up much of the left side and middle of the table, have a tendency to lose electrons in chemical reactions and are therefore good_______ agents. | reducing |
| ________ typically have higher electronegativity values and ________ typically have lower electronegativity values | nonmetals; metals |
| Arrange the following elements in order of decreasing electronegativity. phosphorus, cobalt, oxygen, lithium | oxygen, phosphorus, cobalt, lithium |
| An oxidant is a substance that can accept the electrons from another reagent. Use electronegativity values to determine which one of the following elements is a good oxidant. O, Na, Ni | O |
| Use electronegativity values to determine which of the following elements you would expect to be the best insulator. Cr, Te, Cl | Cl |
| In________ covalent bonds electrons are shared equally between the atoms. In_______ covalent bonds electrons are shared unequally and partial charges develop. | purely; polar |
| Draw the Lewis structure for SiCl2Br2. | ch 6 #4 |
| Exceptions to the octet rule include hydrogen, which is stable with only____ electrons , and boron, which is stable with only_____ electrons . | two; six |
| formal charge = | # of valence e - 1/2(number of bonding electrons) - number of nonbonding electrons |
| when formal charges can be minimized in a lewis structure, that lewis structure is preferred | |
| # 6 ch 6 | |
| An________ is a polyatomic ion that contains oxygen and has a net negative charge. Examples are SO42−, NO3−, and CO32− | oxoanion |
| What is the formal charge on the hydrogen atom in HBr? | 0 |
| What is the formal charge on the bromine atom in HBr? | 0 |
| For a molecule of fluorous acid, the atoms are arranged as HOFO. What is the formal charge on each of the atoms? | 0, 0, +1, -1 |
| Each valid Lewis structure for a compound is called a________ structure. | resonance |
| #11 ch 6 hw | |
| How many resonance structures can be drawn for ozone, O3? | 2 |
| _____,________, AND _________are examples of elements that can have less than an octet of electrons in a covalent compound. | Hydrogen, beryllium, and boron |
| Instead, Be uses its two valence electrons to form_____ bonds, and B uses itse________ valence electrons to form three bonds | two; three |
| Elements in the_______ row of the periodic table and beyond can have more than an octet of electrons in a covalent compound. T | third; |
| how can elements beyond the 3rd period have more than the octet? | This can be explained by the existence of an empty d subshell available to these elements, which allows them to expand their valence to a number greater than eight. |
| How many lone pairs are on the central atom in BCl3? | 0 |
| How many lone pairs are on the central atom of BrF3? | 2 |
| How many electrons should be shown in the Lewis symbol for hydrogen? | 1 |
| #14 ch 5 | |
| what are the prefixes for covalent compounds from 1 - 10? | mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca |
| What is the formula for the compound nitrogen monoxide? What is the formula for the compound tetraphosphorus decoxide? What is the formula for the compound methane? | NO, P4O10, CH4 |
| What is the name of the covalent compound CCl4? What is the name of the covalent compound N2O5? | carbon tetrachloride; dinitrogen pentoxide |
| N2O5; CF4; RnF2; Si3N4 | dinitrogen pentoxide; carbon tetrafluoride; radon difluoride; trisilicon tetranitride |
| XeO3; KBrO; CuSO4 | xenon trioxide; potassium hypobromite; copper (ii) sulfate |
| What is the formula weight of magnesium nitrate, Mg(NO3)2? | 148.3 amu |
| Calculate the formula weight of ethanol, C2H5OH. | 46.1 amu |
| What is the formula weight of sodium carbonate? | 106.0 amu |
| How many moles (of molecules or formula units) are in each sample? 75.56 g CF2Cl2 | .6249 mol |
| How many moles (of molecules or formula units) are in each sample? 23.3 kg Fe (NO3) 2 | 130 mol |
| How many moles (of molecules or formula units) are in each sample? 0.4645 g C8H18 | 4.067 x 10^-3 mol |
| Calculate the mass (in grams) of each sample. 7.1×1025 O3 molecules | 5700 g |
| Calculate the mass (in grams) of each sample. 2.57×1019 CCl2F2 molecules | 5.16 x 10^-3 g |
| Calculate the mass (in grams) of each sample.9 water molecule(s) | 2.693 x 10^-22 g |
| A compound is 40.0% C, 6.70% H, and 53.3% O by mass. Assume that we have a 100.-g sample of this compound. What are the subscripts in the empirical formula of this compound? | C, H, O = 1, 2, 1 |
| The molecular formula mass of this compound is 240 amu . What are the subscripts in the actual molecular formula? | 8, 16, 8 |
| A hydrocarbon is a compound that contains mostly carbon and hydrogen. Calculate the percent composition (by mass) of the following hydrocarbon: C 8 H 18 . | carbon, hydrogen = 84.12%, 15,88% |
| A certain metal hydroxide, M(OH)2, contains 32.8% oxygen by mass. What is the identity of the metal M? | copper |
| A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume you have a 100.-g sample of this compound. How many grams of each element are in this sample? | 80, 20 |
| How many moles of each element are in this sample? | moles of C, moles of H= 6.66, 19.8 |
| Based on the mole ratio you determined in Part C, what is the empirical formula of this compound? | CH3 |
| The molar mass of the compound was found to be 30.069 g/mol. What is the molecular formula? | C2H6 |
| Determine the number of moles of oxygen atoms in each of the following. 5.00 mol H2O2, 2.13 mol N2O, 2.31×10−2 mol H2CO3, 23.3 mol CO2 | A= 10.0 mol B= 2.13 MOL C= 6.93 X 10^-2 MOL D= 46.6 MOL |
| Nitroglycerin (used medically as a vasodilator to treat heart conditions): 15.87%C, 2.22%H, 18.50%N, and 63.41%O. what is the empirical formula | C3H5N3O9 |
| Glucose (a source of energy and metabolic intermediate): 40.00%C, 6.71%H, and 53.29%O.what is the empirical formula? | CH2O |
| #27 ch 5 |
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jackjack109