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MCAT General Chemistry Flashcards

(72 cards)

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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
A substance that contains two or more elements or compounds that retain their chemical identities and can be separated by a physical process
Mixture
26
The formula representing the number and type of constituent atoms in a compound
Molecular formula
27
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
Network solid
28
A compound that contains one or more unpaired electrons and is attracted into a magnetic field
Paramagnetic
29
The maximum number of electrons in any given orbital is 2 and they must have opposite spin
Pauli exclusion principle
30
A horizontal row in the periodic table
Period
31
__is what determines what the element is
Atomic number
32
When does B decay occur?
When an unstable nucleus contains too many neutrons, converts a neutron to a proton and electron, move Right on periodic table
33
When does Positron emission occur?
This occurs when nucleus contains too few neutrons move Left on periodic table
34
If you form ions the radius will_____
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
The amount of energy necessary to remove the least tightly bound electron from an isolated atom is called the atoms __
ionization energy
36
As we move from left to right across a period, or up a group, the ionization energy ___
increases since the valence electrons are more tightly bound
37
The energy associated with the addition of an electron to an isolated atom is known as the atoms ___
electron affinity
38
The halogens have a ___electron addinity value, since the ADDITION of an electron would give them the octet configuration
large NEGATIVE
39
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
POSITIVE electron affinities
40
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
Absolute zero
41
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
Allotropes
42
A process that leads to an increase in the free energy of a system and is therefore NOT spontaneous Grxn is positive
Endergonic
43
A chemical reaction that absorbs heat from the surroundings : Hrxn is positive
Endothermic
44
The total potential energy in a substance due to intermolecular forces and covalent bonds
Enthalpy (H)
45
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
Enthalpy of reaction (Hrxn)
46
A process that leads to a decrease in the free energy of a system and is therefore spontaneous G is negative
Exergonic
47
A chemical reaction that releases energy to the surroundings H is negative
Exothermic
48
The total energy in the universe is conserved: energy is neither created nor destroyed, but may change from one form to another
First law of thermodynamics
49
The energy associated with a chemical reaction that can be used to do work.
Free energy Gibbs (G)
50
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
Hess's law
51
Processes that increase the entropy in the universe are spontaneous
Second law of thermodynamics
52
A reaction in which the product are favored G is negative Ecell is positive
Spontaneous reaction
53
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
Standard heat of formation (Hf
54
State in which T = 298 K P =1 atm and all concentrations are 1 M not STP
Standard state/condition
55
Standard temperature and pressure (STP)
State in which T =273 K (OC) | P= 1 ATM generally used when referring to gases
56
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
State function
57
Melting, freezing, and boiling are all examples of ___
physical changes
58
A key property of a physical change is that no __ bonds are made or broken
Intramolecular bonds are made or broken
59
Physical change affects only the ____ forces between molecules or atoms
Intermolecular forces
60
Going from a solid to a liquid ____
Melting (fusion)
61
Going from a liquid to a solid __
Freezing (crystallization)
62
Liquid to gas ___
vaporization (boiling)
63
Gas to Liquid ___
condensation
64
Solid to gas ____
Sublimation
65
Gas to solid___
Deposition
66
Going from solid -> liquid -> or solid ->L ___ heat, internal Kinetic energy___ Entropy__
Heat is absorbed Internal kinetic energy increase Entropy increases
67
Going from Gas -> liquid ->solid or Gas -> soli ___heat Internal Kinetic energy___ Entropy___
Heat is released Internal KE decrease Entropy decreases
68
The amount of heat required to cause a change of phase depends on two things:
- The type of substance | - The amount of substance
69
Formula for the heat accompanying a phase transition is =
q = n x H(dependent on phase change) q = heat n = number of moles delta H = heat of transition
70
If delta H (heat of transition) and q are positive =
heat is absorbed
71
When a substance absorbs or releases heat one of two things can happen:
- temperature changes - a phase change will occur BUT NOT BOTH AT THE SAME TIME
72
A substance's specific heat is an ____ of that substance and tells us how resistant it is to changing its temperature
Intrinsic property

MCAT (45 decks)

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