Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

NMAT 2022 > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

1
Q

Who developed the atomic Theory

A

John Dalton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is the charge of the electron?

A

-1.6x10^19 C (Robert Millikan)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Established the particle character of cathode rays

A

George Johnstone Stoney

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Established the raisin bread model as a theory of atomic structure

A

J.J. Thompson

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Who discovered that electricity can decompose compounds?

A

Michael Faraday

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Performed an experiment on cathode rays and detected the presence of ions

A

Eugen Goldstein

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Introduced the nuclear model of the atom, used a gold sheet; positive charge in a small region called nucleus

A

Ernest Rutherford

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Discovered the neutron

A

James Chadwick

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the charge of a proton?

A

1.602x10^19 C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Significant observation in chemical periodicity; named groups in triads

A

Johan Wolfgang Dobreiner

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

suggested the law of octaves

A

John Newlands

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Published an independent version of the periodic system; organized in increasing atomic weights

A

Dmitri Ivanovich Mendeleev

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Established the modern periodic table

A

Henry Mosely

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Groups that belong to s/p blocks

A

Group 1A-8A
Alkali metals (except hydrogen)
Alkali earth metals
Aluminum
Carbon
Nitrogen
Oxygen
Halogens
Noble or Inert gasses

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

The transition elements belong to the ___-block

A

d-block

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Inner transition elements belong to the f-block which consists of ______ and ______

A

lanthanide (4f)
actinide (5f)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Periodic Trends that: (2)
L-R : Decrease
T-B : Increase

A

Atomic Radius
Metallicty

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Periodic Trends that: (3)
L-R : Increase
T-B : Decrease

A

Electronegativity
Ionization Energy
Electron Affinity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Qualities that describe the outside appearance of matter

A

Extrinsic properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

depend on the kind of material itself

A

Intrinsic Properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Depend on the amount of matter present

A

Extensive Properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Do not depend on the amount of substance present

A

Intensive properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

structure that is not orderly, melting point is not determined

A

amorphous solids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Viscosity Trends = higher or lower?
Temp
Pressure
IMF

A

higher temp = lower viscosity
higher pressure = higher v
stronger IMF = higher V

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Vapor pressure trends = higher or lower?
Temp
Pressure
IMF

A

higher temp = higher vapor pressure
higher IMF = lower VP
higher VP = lower boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Vapor pressure of a liquid is equal to the external pressure on its surface

A

Boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

when electrons are shared there is a _____ bond between the compounds

A

Covalent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

an _____ bond is formed when non-metals and metals bond together because of a difference in electronegativity

A

ionic bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

A physical combination of two or more distinct chemical substances

A

Mixture

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

A phenomenon wherein a characteristic of suspensions and colloids is their ability to scatter light when passing through a mixture

A

Tyndall effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Suspensions have a particle size larger than ______

A

200nm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Colloids particle size are between ________

A

1-200nm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

The mixture or solution is heated into a vapor and condensed

A

Distillation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

reduction ____ electrons & hydrogen
oxidation ______ electrons & hydrogen

A

reduction = gains
oxidation = release

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

acids: hydrogen ion donor
bases: hydroxide (-OH) donor

A

Arrhenius theory

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

acids: proton donor
bases: proton acceptor

A

Bronsted-Lowry theory

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

acids: electron pair acceptor
bases: electron pair donor

A

Lewis theory

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

SI unit of energy

A

Joule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

1 joule = ___ kg m^2/s^2

A

1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

1 cal = ____ J

A

1 cal = 4.184J

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

KeQ = equilibrium constant formula

A

Keq = (products)^x / (reactants)^y

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

states that “when a system is in equilibrium, the equilibrium shifts so as to undo, in part, the effect of disturbance”

A

Le Chatelier’s principle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

atoms containing radionuclides

A

radioisotope

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

particles are helium atoms

A

alpha emission

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

particles are electrons (0-e)
increase in atomic number

A

beta emission

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

no change in atomic number or mass since rays are uncharged

A

gamma emission

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

(01e) decrease in atomic number

A

positron emission

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

inner shell electron is captured by the nucleus
decrease in atomic number

A

electron capture

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

splitting of heavy nuclei

A

nuclear fission

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

union of light nuclei

A

nuclear fusion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

solutions are ____ mixtures

A

homogenous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

two types of heterogenous mixtures are

A

colloids
suspensions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

elements that have the same number of neutrons but have different number of protons

A

isotones

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

elements that have the same atomic number but different atomic mass number

A

isotopes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

percent composition formula

A

percent composition = (molar mass of element / total molar mass of a compound) x100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

MC molecular geometry on NMAT
Linear:
Tetrahedral:
Bent:

A

Linear: CO2
Tetrahedral: CH4 (methane)
Bent:H2O, SO4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

BF3 geometry

A

trigonal planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

Compounds with tetrahedral arrangement (3)

A

CH4 (methane)
NH3 (ammonia)
H20 (bent)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

Compounds with trigonal bypyramidal geometry (4)

A

PCl5 (phosphorus pentachloride)
SF4 (sulfur tetrafluoride)
ClF3 (Chlorine trifluoride)
I3- (triiodide)

60
Q

Compounds with octahedral arrangement (3)

A

SF6 (Sulfur hexafluoride)
BrF5 (bromine pentafluoride)
XeF4 (xenon tetrafluoride)

61
Q

orbital size and energy level

A

principal quantum number (n)

62
Q

orbital shape

A

angular momentum (l)

63
Q

orbital orientation

A

magnetic quantum number (ml)

64
Q

electron spin direction

65
Q

Electrons will fill the lowest energy level first

A

Aufbau principle

66
Q

no two electrons within an atomy should have an identical set of all four quantum numbers

A

Pauli Exclusion principle

67
Q

electrons will occupy all empty orbitals in a subshell with single electrons having parallel spins before entering half-filled orbitals

A

Hund’s Rule

68
Q

angular momentum
s
p
d
f

A

angular momentum
s = 0
p = 1
d = 2
f = 3

69
Q

maximum electron number
s
p
d
f

A

maximum electron number (half will be the shell or orbital number)
s = 2
p = 6
d = 10
f = 14

70
Q

ml (orientation)
s
p
d
f

A

ml (orientation)
s = 0
p = -1, 0, 1
d = -2, -1, 0, 1, 2
f = -3, -2, -1, 0, 1, 2, 3

71
Q

the s orbital has a _____ shape
the p orbital has a ______ shape

A

s = sphere
p = dumbell

72
Q

the valence electron can be determined according to the ______ of the element

A

group number

73
Q

the more electronegative element gains an electron

74
Q

the less electronegative element loses an electron

75
Q

bond between non-metal and non-metal

A

covalent bond

76
Q

bond between non-metal and metal
an electron is taken by the more electronegative participant

A

ionic bonds

77
Q

______ bonds are formed by fluorine, oxygen or nitrogen

A

hydrogen bonds

78
Q

_____ bonds form a sea of electrons

A

metallic bonds

79
Q

Electrons not equally shared
One part of molecule is more negative or positive

A

Polar molecules

80
Q

Electrons equally shared
No one part of molecule is more negative or positive

A

Non-polar molecules

81
Q

Polar Molecules ____
Non-Polar molecules ____

A. hydrophobic
B. hydrophilic

A

Polar Molecules: HYDROPHILIC
Non-Polar molecules HYDROPHOBIC

82
Q

metal cations to delocalized electrons

A

metallic bonds

83
Q

cations to anions

A

ionic bond

84
Q

partially charged cation to partially charged anion

A

polar covalent bonds

85
Q

nuclei to shared electrons

A

non polar covalent bonds

86
Q

partially oppositely charged ions

A

dipole-dipole attraction

87
Q

weakest intermolecular forces of attraction

A

london dispersion attraction

88
Q

greater molecular weight = _______ london dispersion forces

89
Q

higher boiling point = _______ vapor pressure

A

higher boiling point = lower vapor pressure

90
Q

higher boiling point =

higher: (3)
lower: (2)

A

higher boiling point =

higher: (3) IMF, MW, surface area
lower: (2) branching, VP

91
Q

2 or more simpler substances (elements) combine to give a compound

92
Q

Compound is broken down into simpler substances (elements)

A

Decomposition

93
Q

Atom or group of atoms is replaced by another atom or group
A + BC = AC + B or AB + C

A

Single Replacement

94
Q

Solid compound is formed
2 soluble compounds are mixed
AB+ CD = AD + BC

A

Double Replacement

95
Q

Reaction between hydrocarbon and oxygen to produce carbon dioxide, water and heat.
An exothermic reaction

A

Combustion

96
Q

An acid reacts with a base to produce salt and water

HA + BOH –> H2O + BA

A

Neutralization

97
Q

Electron transfer occurs

A

Reduction-Oxidation

98
Q

an oxidizing agent = _____ electrons

A

an oxidizing agent = gains electrons

99
Q

a reducing agent ______ electrons

A

a reducing agent loses electrons

100
Q

True or False
there are no attractive or repulsive forces between particles of real gases

A

False
there are no attractive or repulsive forces between particles of Ideal gases

101
Q

Real gases have ____ volume whereas ideal gases have ____ volume

A

Real gases have small volume whereas ideal gases have no volume

102
Q

real gases = _____ collision
ideal gases = ______ collision

A

real gases = inelastic collision
ideal gases = elastic collision

103
Q

volume is _______ proportional to pressure

A

volume is inversely proportional to pressure
high V = low P
low V = high P

104
Q

volume is directly proportional to ______ and _______

A

temp and number of moles

105
Q

Ideal Gas law formula

106
Q

Combined gas law formula

A

P1V1/T1 = P2V2/T2

107
Q

At constant V, as pressure increases, temperature increases

A

Gay-Lussac’s law

108
Q

Gay-Lussac’s law formula

A

P1/T1 = P2/T2

109
Q

At constant P, as volume increases, temp increases

A

Charles Law

110
Q

Charles Law Formula

A

V1/T1 = V2/T2

111
Q

At constant T, as pressure increases, volume decreases

A

Boyles Law

112
Q

Boyle’s Law formula

113
Q

How many steps are there to convert mol to mol

A

1 step (mol of A to mol of B)

114
Q

How many steps are there to convert mol to grams?

A

2 steps (mol A –> mol B –> gB)

115
Q

How many steps are there to convert grams to mol?

A

2 steps (gA –> mol A –> mol B)

116
Q

How many steps are there to convert grams to grams?

A

3 steps (gA –> mol A –> mol B –> gB)

117
Q

What is the first step in limiting and excess reactants?

A

identify ER and LR (divide total number of mols by mols in balanced equation or do mol to gram conversions with product)

118
Q

How to compute for excess reactants?

A

Total reacted - theoretical reacted = leftover

119
Q

Formula of percent yield

A

%yield = A/T x 100

120
Q

measurement of randomness of molecules

A

Entropy (∆S)

121
Q

amount of heat evolved or absorbed in a reaction carried out at constant pressure

A

Enthalpy (ΔH)

122
Q

First Law of Thermodynamics

A

Energy can never be created or destroyed

Energy can only be converted from one form into another

123
Q

Second Law of Thermodynamics

A

Total entropy of the universe always increases

Every spontaneous change is accompanied by an increase in entropy

124
Q

Third Law of Thermodynamics

A

At absolute zero, the entropy of a perfect crystalline substance may be taken as zero

125
Q

Exothermic or Endothermic?
Formation of products is more favorable
Formation of reactants is more favorable

A

Formation of products is more favorable - Exothermic
Formation of reactants is more favorable - Endothermic

126
Q

Reaction is spontaneous

A

Exothermic reaction

127
Q

Reaction is not spontaneous
Energy absorbed

A

Endothermic reaction

128
Q

The relationship between heat energy and temperature is different for every material, and the ___________ is a value that describes how they relate.

A

specific heat

129
Q

formula for heat

130
Q

free energy change for a reaction

A

Gibbs free energy (ΔG)

131
Q

reaction that favors the formation of products at the conditions under which the reaction is occurring

A

Spontaneous reaction

132
Q

reaction that does not favor the formation of products at the given set of conditions

A

Nonspontaneous reaction:

133
Q

formula for change in Gibb’s free energy

A

ΔG = ΔH - TΔS

134
Q

ΔG < 0

135
Q

Solution with solute that dissolves until it is unable to dissolve anymore
Leaves undissolved substances at the bottom

A

Saturated Solution

136
Q

Less solute than the saturated solution
Solution completely dissolves
No remaining substances

A

Unsaturated Solution

137
Q

Has more undissolved solute than the saturated solution Tendency to crystallize and precipitate

A

Supersaturated Solution

138
Q

acids turn litmus paper from ____ to _____

A

blue to red

139
Q

Molarity formula

A

M = moles of solute / liters of solution

140
Q

Molality formula

A

m = moles of solute / kg solvent

141
Q

normality formula

A

N = #H+ or OH- /L of solution

142
Q

Mass percent solution

A

mass solute / mass of solution x100

143
Q

mole fraction

A

moles of solute/moles of solution

144
Q

Rate Law Formula

A

(Concentration)F - (Concentration)I / change in time

145
Q

Chemical Equilibrium Formula

A

Kc = (C)^c (D)^d / (A)^ab (B)^b

NMAT 2022 (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions