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Chem Test-Dec. 2
Chapter 8
| Question | Answer |
|---|---|
| Every substance is either an element or a ( ) | compound |
| A compound is either ( ) or ionic in nature | molecular |
| Most molecular compounds are composed of two or more ( ) | nonmetals |
| Molecules consisting of two or more atoms are ( ) molecules | diatomic |
| The chemical formula of a molecular compound is a ( ) | molecular formula |
| Molecular compounds tend to have ( ) melting and boiling points | low |
| Ionic compounds tend to have ( ) melting and boiling points | high |
| A molecular formula shows how many ( ) of each element contains | atoms |
| A molecular formula does not indicate the ( ) of the molecule | structure |
| *T-F* A diatomic molecule contains two or three atoms | Never True |
| *T-F* Molecular compounds have relatively high boiling points | Never True |
| *T-F* The molecular structure of carbon dioxide is one carbon atom with two oxygen atoms on opposite sides of it | Always True |
| *T-F* A molecule contains two atoms | Sometimes True |
| Molecule | an electrically neutral group of atoms joined together by covalent bonds |
| Molecular Compound | a compound composed of molecules |
| Covalent Bond | joins atoms held together by sharing electrons |
| Diatomic molecule | a molecule consisting of two atoms |
| Molecular Formula | shows the kinds and numbers present in a molecule of a compound |
| When atoms share electrons to gain the electron configuration of a noble gas, the bonds formed are ( ) | covalent |
| A shared pair of valence electrons constitutes a ( ) covalent bond | single |
| Pairs of valence electrons that are not shared between atoms are called ( ) | unshared pairs |
| Sometimes two or three pairs of electrons may be shared to give ( ) covalent bonds | double/triple |
| A ( ) is a bond in which only one of the atoms provides the pair of bonding electrons | coordinate covalent bond |
| ( ) is required to break the bond between two atoms | energy |
| The total energy required to break covalently bonded atoms is ( ) | bond dissociation energy |
| When a molecule or ion has two or more valid electron dot formulas, each formula is referred to as a ( ) | resonance structure |
| *T-F* The modern interpretation of resonance is that electron pairs rapidly flip back and forth between the various electron dot structures | Never True |
| *T-F* The compound NH3 contains two double covalent bonds | Never True |
| *T-F* The chemical formulas of molecular compounds show the number and type of atoms in each molecule | Always True |
| *T-F* A molecule of bromine has six unshared pairs of electrons | Always True |
| *T-F* Carbon forms four single covalent bonds with other bond | Sometimes True |
| *T-F* A bond in which one atom contributes both bonding electrons is called a polyatomic covalent bond | Never True |
| single covalent bond | a chemical bond in which only one pair of electrons is shared by two bonded atoms |
| structural formula | a chemical formula that shows the arrangement of atoms in a molecule or polyatomic ion |
| bond dissociation energy | the amount of energy required to break a covalent bond between atoms |
| polyatomic ion | a tightly bound group of atoms that has a positive charge and behaves as a unit |
| coordinate covalent bond | a chemical bond in which only one pair of electrons is shared by two bonded atoms |
| the quantum mechanical model of bonding assumes that atomic orbitals can overlap to produce ( ) | molecular orbitals |
| A molecular orbit that can be occupied by two electrons of a covalent bond is called a ( ) | bonding orbital |
| A bonding orbital's energy is ( ) than that of the atomic orbitals from which it formed | lower |
| When two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting two atomic nuclei, a ( ) bond is formed | sigma |
| When atomic orbitals overlap side by side, they produce ( ) bonds | pi |
| Electron dot structures fail to reflect the ( ) shapes of molecules. | 3-D |
| ( ) states that because electron pairs repel, molecular shape adjusts so the valence-electron pairs are as far apart as possible | VSEPR Theory |
| A way to describe molecules that provides information about both molecular bonding and molecular shape is ( ) | orbital hybridization |
| *T-F* Unshared pairs of electrons affect the shape of molecules | Always True |
| *T-F* Molecular orbitals involve pi bonding | Sometimes True |
| *T-F* Bonding orbital is a molecular orbital whose energy is higher than that of the atomic orbitals from which it is formed | Never True |
| *T-F* With hybridization, several atomic orbitals overlap to form the same total number of equivalent hybrid orbitals | Always True |
| *T-F* Sigma and pi bonds are found in the same molecule | Sometimes True |
| *T-F* The methane molecule has four orbitals with tetrahedral angles of 109.5 | Always True |
| Sigma Bond | a bond formed when two atomic orbital combine to form a molecular orbital that is symmetrical to the two atomic nuclei |
| Pi Bond | A bond in which the bonding electrons are most likely to be found in the sausage-shaped regions above and below the nuclei of the bonded atoms |
| VSEPR Theory | states that because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible |
| hybridization | a process in which several atomic orbitals overlap to form the same number of equivalent hybrid orbitals |
| linear molecule | a term used to describe the shape of certain molecules such as CO2 |
| When like atoms are joined by a covalent bond, the bonding electrons are shared equally and the bond is ( ) | nonpolar |
| When the atoms in the bond are not the same, the bonding electrons are shared unequally, and the bond is ( ) | polar |
| The degree of polarity of a bind between any two atoms is determined by consulting a table of ( ) | electronegatives |
| The attractions between opposite poles of polar molecules are called | dipole interactions |
| When a hydrogen covalenty bonded to a very electronegative atom, such as oxygen, nitrogen, fluorine, is also weakly bonded to an unshared electron pair of another electronegative atom, it is called a | hydrogen bond |
Created by:
emmazeitler42