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Test 1
Nursing Anesthesia - Physics & Chemistry - Testable pack #1
| Question | Answer |
|---|---|
| A number of protons found in the nucleus of an atom account for the… | The atomic number |
| Matter composed of atoms that all have the same atomic numbers | Element |
| This is smallest unit of an element to retain all the chemical properties of that element | Atom |
| Electrons, protons, and neutrons are that kind of particles | Subatomic particles |
| This particle in the nucleus with a positive charge of +1 & an atomic mass number of 1 | Proton |
| This is a non-charged nuclear particle with the same mass as the proton | Neutron |
| This is a negatively charged particle with a mass 1/1837 of that of a proton | Electron |
| This is the electromagnetic force involved with the electron is held around the nucleus by | Atomic forces |
| Signifies the actions of the electrons in orbit | Quantum numbers |
| Atomic number is based on | the number of protons |
| The atomic mass is calculated | By the total of the number of protons + the number of neutrons |
| Every proton or neutron has a mass of | 1 amu. Amu = atomic mass unit |
| Isotopes have the same number of protons, same atomic number, differ in the number of neutrons which causes… | Different atomic mass |
| With Isotopes, Protons = | electrons |
| With Isotopes the chemical behavior is determined | Mainly by electrons |
| Heavier isotopes react (quicker/slower) | slower |
| This defines the greater the proton/neutron ratio the less stable the nucleus… | Nuclear decay |
| These contain a net electrical charge | Ion |
| These are negative charge ions that are attracted to anodes | Anion |
| These are positive charge that are attracted to cathodes | Cation |
| This is an example of mass spectrometry used in anesthesia | Gas analyzer |
| This is determines mass/charge ratio | Mass spectrometry |
| In mass spectrometry, this is the sample must be… | in Gas form (vaporized) |
| In mass spectrometry, sample is broken down or another definition for this | Ionized. This ionized sample pass by a magnetic field and pulled the ions causing a curve |
| T/F The lighter ions curve farther than the heavier ones | True |
| The ion mass/charge ratio is calculated based on the variance of | deflection |
| Valence shell located here | within the outermost energy level of an atom |
| Elements with a full outer shell are very (unreactive or reactive). | Very Unreactive |
| Elements with an almost full or almost empty outer shells tend to be very (non-reactive or reactive). | Very Reactive |
| The atoms that travel furthest from nucleus have the greatest energy and … | Determine physical properties |
| This occurs when atoms combine in such a way to have eight electrons in their valence shells | Octet rule |
| Octet rule is the same as… | Same as noble gas |
| Molecular formation formed by | bonds |
| This is when atoms attempt to achieve stability | Molecular formation |
| With Molecular formation stability is created by.. | A full outer shell |
| Molecular formation is done by forming bonds with other atoms, which requires >this< | Requires energy |
| This is the energy required to break a bond | Kcal/mole |
| This type of bond Share of electrons between atoms | Covalent Bonds |
| With pure covalent bond the electronegativity difference is this amount | Zero |
| Covalent Bonds are usually (non-soluble/soluble) | Non-soluble |
| Covalent Bonds are electrically (non-conductive/conductive) | Non-conductive |
| This defines the affinity for atom to bind electrons | Electronegativity |
| Electronegativity of Oxygen | 3.5 |
| Electronegativity of Carbon | 2.5 |
| Electronegativity of Hydrogen | 2.1 |
| This is the example of covalent bond | Water. Oxygen has slight negative charge. Hydrogen atoms have slight positive charge. Electrostatic attraction exists between oxygen of one molecule and hydrogen of another molecule. |
| This bond occurs when electron is given up to another | Ionic bonds. One atom negative, one atom positive. Negative atom is then attracted to the positive atom. |
| In ionic bond, negative atom is then attracted to the positive atom due to … | the electrostatic forces |
| This is an example of an ionic bond | Common table salt, Na+ & Cl- |
| Ionic Bonds are (Weaker or Stronger) than hydrogen bonds, and are similar to what | Stronger, similar to covalent bonds |
| T/F Pure ionic bond doesn’t exist. | True |
| T/F Ionic bonds have a high electronegativity. | False, ionic bonds have zero electronegativity |
| These bonds TEND TO BE SOLUABLE IN WATER | Ionic Bond |
| This bond results from 2 ionized groups of opposite charge or polarized molecules | Electrostatic bonds |
| This is a property of gas | Density |
| Density is calculated by | = mass/volume |
| Gas has no given … | volume |
| Gas Density is determined by | the container it is in |
| Density is the physical property that allows for the proper function of what anesthesia system | the open scavenger system |
| These are determined by how the properties of a liquid solution change depending on the concentration of the solute in it. | Colligative Properties |
| T/F Colligative properties includes Vapor pressure, Freezing point depression, Boiling point elevation, and Osmotic pressure | True |
| This is the solution shows a decrease in melting point as the amount of solute is increased. | Freezing point |
| This is difference between the freezing points of a pure solvent and a solution mixed with a solute. | Freezing point depression |
| This is directly proportional to the molal concentration of the solution according to the equation | Freezing point depression Example:Kf for water is 1.86 K•kg/mol, per mole of solute dissolved in a kilogram of water the freezing point depression is 1.86 kelvins |
| With the boiling point elevation, the solution shows an increase in boiling point as … | the amount of solute is increased. |
| A solution will have a higher boiling point than | that of a pure solvent. |
| This is the pressure produced by a solution in a space that is enclosed by a differentially permeable membrane | Osmotic Pressure |
| With the greater the solute and the greater, the osmotic pressure greater the … | concentration gradient |
| 2 Examples where Osmotic Pressure is involved | B/P, cell hydration |
| This is the elastic collisions with walls of a container | Gas Vapor Pressure |
| Related to vapor pressure , the number X2 = | double number of collisions |
| Double the volume (space) , <this amount >of collisions | double number of collisions |
| The more molecules hit wall of the container | Faster molecules are moving |
| With these, the faster molecules hit walls with more force | Larger molecules |
| This defines a solution of a solid non-volatile solute in a liquid solvent shows a decrease in vapor pressure above the solution as the amount of solute is increased. | Vapor Pressure |
| This is formed by molecules escaping from a liquid | Vapor |
| When a substance is place in an evacuated, closed container. The pressure in the space above the liquid would increase from zero and eventually stabilize at a constant value, this is describes... | Vapor pressure |
| Vapor pressure is measured by this = …. | 1 torr = 1 mm Hg |
| This relates to the rate atoms & molecules escape from a liquid. | Vapor pressure |
| 3 things that are seen with the more volatile a substance is | 1) Molecules will escape faster from a liquid 2) It will have a lower boiling point 3) The higher the vapor pressure of a substance |
| 2 gas with high vapor pressures | Isoflurane, sevoflurane |
| This gas has the highest vapor pressures | Desflurane |
| This is the point were the pressure of a gas is equal to its liquid form in a closed container | Saturation vapor pressure |
| Related to Saturation vapor pressure in an open container >>this<< pressure is the opposing force | Atmospheric pressure |
| This account for the number of calories needed to convert 1 g of liquid to vapor | Latent heat vaporization |
| T/F The temperature of the remaining liquid will drop as vaporization proceeds | True |
| This is a product of vaporization | Heat |
| With vaporization if no heat is added, the heat is taken from … | the substance |
| Vapor Pressure in a closed container is independent of this pressure | atmospheric pressure |
| This depends only on the physical characteristics of the liquid, and its temperature. | Vapor Pressure |
| The more volatile the agent, the more … | energy (heat) is created (used) |
| This gas is inert at room temperature | Nitrous oxide |
| Nitrous oxide is liquid at >>this<< temperature and it s pressures is… | Room temperature, pressure greater than 745 PSI |
| T/F Nitrous oxide tanks need to be changed when they reach a pressure of 790 PSI | False, 745 PSI In theory: you may only have gas left in the tank, which won’t last long |
| This type of energy is energy of motion | kinetic |
| This type of energy is involved chemical bonds | chemical |
| This type of energy due to its charge | electrical |
| This type of energy due to its heat | thermal |
| This type of energy due to the instability of the nuclei of its atoms | nuclear |
| This type of energy due to the position of the object relative to other objects | potential |
| This defines the total inflow of energy into a system must equal the total outflow of energy from the system, plus the change in the energy contained within the system | Conservation of energy |
| What can be converted from one form to another, but it cannot be created or destroyed | Energy |
| This = energy added (heat) – work done | Amount of energy of a system |
| T/F The energy available after a chemical reaction is less than that at the beginning of a reaction | True |
| This is the amount of unusable energy within a system | Entropy |
| As energy is transferred from one form to another, some is lost as heat; and… | entropy increases. Continuous motion without a change of energy is impossible |
| If there is no change of energy within a system, the system would remain … | constant |
| T/F Movement of heat only flows in one direction from cold to hot. | False, from hot to cold |
| T/F Flow of heat stops at absolute zero. | True |
| Conduction, convection, radiation are all type of… | Heat transfer |
| This is not a true heat transfer mechanism | Evaporation |
| This is heat loss by transmission of heat across matter | Conduction |
| Denser substances are usually better conductors; metals are .. | excellent conductors. |
| In Conduction, heat lost is through | direct contact |
| In Radiation, heat loss due to … | temperature gradient |
| Related to human temp. , this gradient would occur with temperatures less than.. | 98.6 F |
| 2 Example of Evaporation related to human temperature regulation | Sweating, Respiration |
| Heat Loss related to Convection is due to… | Constant movement of one of the surfaces |
| With the example of the Wind: as your body heat warms up the air around you, the wind replaces that air with cooler air thus creating | a greater temperature gradient. Water also works in the same manner |
| This is an example of reverse convection | convention oven. As the turkey cools the air around it, the fan replaces the air around the turkey with warm air, creating a less a temperature gradient. |
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honeybeeforeman
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