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MCAT > MCAT General Chemistry > Flashcards

MCAT General Chemistry Flashcards

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MCAT flashcards
1
Q

__is equivalent to the number of protons in the nucleus of an atom

A

Atomic number (Z)

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2
Q

__is the principle that atomic orbitals are filled one at a time, starting with the orbital that has the lowest energy and then filling upwards

A

Aufbau principle

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3
Q

A model of the distribution of electrons in an atom based on the assumption that the electron in a hydrogen atom is in one of a limited number of orbits

A

Bohr model

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4
Q

The temperature at which the vapor pressure of a liquid is equal to the external or atmospheric pressure

A

Boiling point

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5
Q

The energy needed to homolytically break a bond to give two atoms in the gas phase

A

Bond-dissociation energy/ Enthalpy

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6
Q

A covalent bond formed as a result of a Lewis acid-base reaction, most often formed between a metal atom and a nonmetal atom

A

Coordinate covalent bond

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7
Q

A compound in which one or more ligands are coordinated to a metal atom

A

Coordination compound

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8
Q

A three-dimensional solid formed by regular repetition of the packing of atoms, ions, or molecules

A

Crystal

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9
Q

A substance in which the electrons are all paired

A

diamagnetic

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10
Q

Anything with two equal but opposite electrical charges, such as the positive and negative ends of a polar bond or molecule

A

Dipole

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11
Q

Capable of being drawn into sheets or wires without breaking; this is a property of metals

A

Ductile

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12
Q

The energy given off when a neutral atom in the gas phase picks up an electron to form a negatively charged ion

A

Electron affinity

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13
Q

A type of beta decay where the nucleus of an atom captures an electron and converts a nuclear proton into a neutron

A

Electron capture

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14
Q

A vertical column of elements in the periodic table

A

Family

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15
Q

A high energy SHORT wavelength form of electromagnetic radiation emitted by the nucleus of an atom that carries off some of the energy generated in a nuclear reaction

A

Gamma ray

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16
Q

A vertical column or family on the periodic table can also be called a __

A

group

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17
Q

Rule for placing electrons in equal energy orbitals which states that:
-Electrons are added with parallel spins until each of the orbitals has one electron, before a second electron is placed in a given orbital

A

Hund’s rule

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18
Q

A short lived separation of charge, or dipole, of a nonpolar atom or molecule caused by the electrostatic influence of a nearby polar atom or ion

A

Induced dipole

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19
Q

An atom or molecule that accepts a pair of electrons to form a new coordinate covalent bond, almost always a metal, positively charged ion, or both

A

Lewis acid

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20
Q

An atom or molecule that donates a pair of electrons to form a new coordinate covalent bond. Almost always a nonmetal, with a pair of nonbonding electrons

A

Lewis base

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21
Q

Intermolecular forces that arise from interactions between an instantaneous dipole/induced dipole pair. Typically, these are the weakest of all intermolecular forces.

A

London dispersion forces

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22
Q

Something that can be hammered, pounded, or pressed into different shapes without breaking (common metal property)

A

Malleable

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23
Q

The total number of protons and neutrons in the nucleus of an atom

A

Mass number

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24
Q

The temeprature at which the solid and liquid phase of a substance are in equilibrium at a aprticular external pressure

A

Melting point

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25
Q

A substance that contains two or more elements or compounds that retain their chemical identities and can be separated by a physical process

A

Mixture

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26
Q

The formula representing the number and type of constituent atoms in a compound

A

Molecular formula

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27
Q

A solid, such as diamond, in which every atom is covalently bonded to its nearest neighbors to form an extended array of atoms rather than individual molecules

A

Network solid

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28
Q

A compound that contains one or more unpaired electrons and is attracted into a magnetic field

A

Paramagnetic

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29
Q

The maximum number of electrons in any given orbital is 2 and they must have opposite spin

A

Pauli exclusion principle

30
Q

A horizontal row in the periodic table

A

Period

31
Q

__is what determines what the element is

A

Atomic number

32
Q

When does B decay occur?

A

When an unstable nucleus contains too many neutrons, converts a neutron to a proton and electron, move Right on periodic table

33
Q

When does Positron emission occur?

A

This occurs when nucleus contains too few neutrons move Left on periodic table

34
Q

If you form ions the radius will_____

A

Decrease as electrons are removed (because the ones that are left will be held closer to nucleus)
-Increase as electrons are added

Ex: X+

35
Q

The amount of energy necessary to remove the least tightly bound electron from an isolated atom is called the atoms __

A

ionization energy

36
Q

As we move from left to right across a period, or up a group, the ionization energy ___

A

increases since the valence electrons are more tightly bound

37
Q

The energy associated with the addition of an electron to an isolated atom is known as the atoms ___

A

electron affinity

38
Q

The halogens have a ___electron addinity value, since the ADDITION of an electron would give them the octet configuration

A

large NEGATIVE

39
Q

The noble gases and alkaline earth metals have a ___affinity because added electron begins to fill a new level or sublevel and destabilizes the electron configuration

A

POSITIVE electron affinities

40
Q

The temperature (-273.15C or 0K) at which the volume and pressure of an ideal gas extrapolate to zero according to the ideal gas law

A

Absolute zero

41
Q

Forms of a pure element with which different structures and therefore different chemical and physical properties, such as O2 and O3 or diamond and graphite

A

Allotropes

42
Q

A process that leads to an increase in the free energy of a system and is therefore NOT spontaneous Grxn is positive

A

Endergonic

43
Q

A chemical reaction that absorbs heat from the surroundings : Hrxn is positive

A

Endothermic

44
Q

The total potential energy in a substance due to intermolecular forces and covalent bonds

A

Enthalpy (H)

45
Q

The change in the enthalpy that occurs during a chemical reaction. The difference between the sum of the enthalpies of the products and the reactants

A

Enthalpy of reaction (Hrxn)

46
Q

A process that leads to a decrease in the free energy of a system and is therefore spontaneous G is negative

A

Exergonic

47
Q

A chemical reaction that releases energy to the surroundings H is negative

A

Exothermic

48
Q

The total energy in the universe is conserved: energy is neither created nor destroyed, but may change from one form to another

A

First law of thermodynamics

49
Q

The energy associated with a chemical reaction that can be used to do work.

A

Free energy Gibbs (G)

50
Q

The heat given off or absorbed in a chemical reaction does not depend on whether the reaction occurs in a single step or in many steps

A

Hess’s law

51
Q

Processes that increase the entropy in the universe are spontaneous

A

Second law of thermodynamics

52
Q

A reaction in which the product are favored
G is negative
Ecell is positive

A

Spontaneous reaction

53
Q

The change in the enthalpy that occurs during a chemical reaction that leads to the formation of one mole of a compound from its elements in their standard states at standard conditions

A

Standard heat of formation (Hf

54
Q

State in which T = 298 K
P =1 atm
and all concentrations are 1 M not STP

A

Standard state/condition

55
Q

Standard temperature and pressure (STP)

A

State in which T =273 K (OC)

P= 1 ATM generally used when referring to gases

56
Q

A quantity whose value depends only on the state of the system and not its history; X is a state ufnction, if and oly if, the value of deltaX does not depend on the path used to go from the initial to the final state of the system

A

State function

57
Q

Melting, freezing, and boiling are all examples of ___

A

physical changes

58
Q

A key property of a physical change is that no __ bonds are made or broken

A

Intramolecular bonds are made or broken

59
Q

Physical change affects only the ____ forces between molecules or atoms

A

Intermolecular forces

60
Q

Going from a solid to a liquid ____

A

Melting (fusion)

61
Q

Going from a liquid to a solid __

A

Freezing (crystallization)

62
Q

Liquid to gas ___

A

vaporization (boiling)

63
Q

Gas to Liquid ___

A

condensation

64
Q

Solid to gas ____

A

Sublimation

65
Q

Gas to solid___

A

Deposition

66
Q

Going from solid -> liquid -> or solid ->L
___ heat,
internal Kinetic energy___
Entropy__

A

Heat is absorbed
Internal kinetic energy increase
Entropy increases

67
Q

Going from Gas -> liquid ->solid or Gas -> soli
___heat
Internal Kinetic energy___
Entropy___

A

Heat is released
Internal KE decrease
Entropy decreases

68
Q

The amount of heat required to cause a change of phase depends on two things:

A
  • The type of substance

- The amount of substance

69
Q

Formula for the heat accompanying a phase transition is =

A

q = n x H(dependent on phase change)

q = heat
n = number of moles
delta H = heat of transition

70
Q

If delta H (heat of transition) and q are positive =

A

heat is absorbed

71
Q

When a substance absorbs or releases heat one of two things can happen:

A
  • temperature changes
  • a phase change will occur

BUT NOT BOTH AT THE SAME TIME

72
Q

A substance’s specific heat is an ____ of that substance and tells us how resistant it is to changing its temperature

A

Intrinsic property

MCAT (45 decks)

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