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General Chemistry - MCAT > Class 1 > Flashcards

Class 1 Flashcards

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1
Q

prefix - nano

A

10-9

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2
Q

prefix - micro

A

10-6

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3
Q

prefix - mili

A

10-3

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4
Q

prefix - centi

A

10-2

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5
Q

prefix - kilo

A

103

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6
Q

prefix - mega

A

106

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7
Q

angstrom

A

unit of length

10-10 m

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8
Q

density formula

A

mass / volume

kg/m3 or g/cm3

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9
Q

density of water

A

1 g/cm3

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10
Q

empirical formula

A

reducing the molecular formula to the smallest possible ratio

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11
Q

ammonium

A

NH4+

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12
Q

hydronium

A

H3O+

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13
Q

acetate

A

CH3CO2-

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14
Q

bicarbonate

A

HCO3-

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15
Q

cyanide

A

CN-

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16
Q

hydroxide

A

OH-

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17
Q

nitrate

A

NO3-

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18
Q

nitrite

A

NO2-

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19
Q

perchlorate

A

ClO4-

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20
Q

carbonate

A

CO32-

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21
Q

sulfate

A

SO42-

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22
Q

sulfite

A

SO32-

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23
Q

phosphate

A

PO43-

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24
Q

what is a mole

A

6.02 x 1023 entities (Avogadro’s number)

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25
Q

how to calculate the # of moles

A

mass in grams / molecular weight

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26
Q

what is molarity

A

of moles of solute / # litres of solution

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27
Q

Law of Conservation of Mass

A

amount of mass does not change in a chemical reaction

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28
Q

limiting reagent

A

limits how much product a reaction can produce

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29
Q

group 1 metals oxidation state

A

+1

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30
Q

group 2 metals oxidation state

A

+2

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31
Q

fluorine oxidation state

A

-1

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32
Q

hydrogen oxidation states

A

+1 when bonded to something more electroneg. than carbon

-1 when bonded to something less electroneg. than carbon

0 when bonded to carbon

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33
Q

oxygen oxidation state

A

-2

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34
Q

oxygen’s oxidation state exception in peroxides

A

-1 instead of -2

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35
Q

what never assumes a neg oxidation state

A

metals

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36
Q

what does a central nucleus contain

A

protons and neutrons (aka nucleons)

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37
Q

how are electrons held in the atom

A

by the electrostatic attraction of the positively charged nucleus

38
Q

what is the atomic number

A

of protons in the nucleus of an atom

39
Q

what is the atomic mass number

A

of neutrons + # of protons

40
Q

what is an isotope

A

two atoms of the same element with a different # of neutrons

41
Q

what is the atomic weight of an element

A

a weighted average of the masses of the element’s isotopes

42
Q

strong nuclear force

A

holds the protons + neutrons together in a nucleus

43
Q

unstable nuclei are..

A

radioactive

44
Q

radioactive decay

A

alternating the # of protons/neutrons or lowering of energy

45
Q

alpha particle

A

2 neutrons + 2 protons

emitted from parent nucleus

46
Q

types of beta decay

A

beta -

beta +

electron capture

47
Q

characteristic of beta decay

A

conversion of a neutron into a proton

48
Q

are beta or alpha particles more dangerous

A

beta - smaller + have more energy

49
Q

beta - decay

A

too many neutrons: conversion of a neutron into a proton - ejected from the nucleus

atomic number is now 1 greater

mass number remains the same

50
Q

which is the most common type of beta decay

A

beta -

51
Q

beta + decay

A

too few neutrons: conversion of a proton → neutron and a positron

atomic number is now 1 less

mass number is the same

52
Q

positron vs electron

A

positron is the electron’s antiparticle

identical to electron but with a positive charge

53
Q

electron capture

A

increase # of neutrons by capturing an electron from the closest electron shell & uses it to convert a proton into a neutron

atomic number is now 1 less

mass number is the same

54
Q

gamma decay

A

when a nucleus relaxes to its ground state, it emits photons of electromagnetic radiation (aka gamma photons)

55
Q

characteristics of gamma photons

A

very high frequency and energy

no mass or share

ejection from nucleus doesn’t change the atomic number or mass number

56
Q

half life equation

A
57
Q

nuclear binding energy

A

energy that was released when the nucleons were bound together (by the strong force to form nucleus)

58
Q

the greater the binding energy per nucleon..

A

the more stable the nucleus is

59
Q

mass defect

A

when nucleons bind to form the nucleus, some mass is converted to energy so the mass of the combined nucleus is less than the sum of the nucleons masses

60
Q

for a stable nucleus, the mass defect will always be..

A

positive

61
Q

mass defect =

A

total mass of separate nucleons - mass of nucleus

62
Q

Einstein & nuclear binding energy formula

A
63
Q

energy of photon formula

A
64
Q

absorption of a photon - energy change

A

positive energy change

65
Q

emission of a photon - energy change

A

negative energy change

66
Q

limitation of Bohr’s model

A

only applies to atoms with only one electron

67
Q

what is an orbital

A

a 3D region around the nucleus where electrons are most likely to be found

68
Q

s subshell

A

one spherical orbital

69
Q

p subshell

A

3 dumbbell shaped orbitals

70
Q

Aufbau’s principle

A

electrons occupy the lowest energy orbitals available

sub shells are filled in order of increasing energy

71
Q

Hund’s rule

A

electrons in the same subshell occupy available orbitals before pairing up

72
Q

Pauli exclusion principle

A

no more than 2 electrons in any orbital

73
Q

diamagnetic

A

an atom that has all of its electrons spin paired

no net magnetic field → will be repelled by a produced magnetic field

74
Q

paramagnetic

A

when an atom’s electrons are not all spin paired

attracted to externally produced magnetic fields

75
Q

isoelectronic

A

when 2 atoms have the same electron configuration

76
Q

atomic radius pattern

A

decreases across a period

increases down a group

77
Q

ionic radius pattern

A

radius decreases as electrons are removed (cation)

radius increases as electrons are added (anion)

78
Q

what is ionization energy

A

energy needed to remove an electron from an atom

79
Q

ionization energy pattern

A

increases across a period

decreases down a group

80
Q

what is electron affinity

A

amount of energy released when an electron is added

81
Q

electron affinity pattern

A

electron affinity becomes more negative as we move across a period and up a row (except noble gases)

82
Q

what is electronegativity

A

tendency for an atom to attract electrons

83
Q

electronegativity pattern

A

increases across a period

decreases down a group

84
Q

order of electronegativity

A

uncle F O N Cl

Br I S C H

85
Q

what is acidity (trend)

A

how well a compound donates protons/excepts electrons

86
Q

acidity pattern

A

increases across a period

increases down a group

87
Q

number of protons =

A

atomic number

88
Q

number of neutrons =

A

atomic mass - atomic number

89
Q

Planck’s constant

A

6.6 x 10-34 J.s

90
Q

speed of light = c

A

3 x 108

General Chemistry - MCAT (6 decks)

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