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INORGANIC CHEMISTRY > PART 1 > Flashcards

PART 1 Flashcards

1
Q

The science that describes matter—its properties, the changes it undergoes, and the energy changes that accompany those processes

A

Chemistry

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2
Q

Chemistry is also called the ___ science.

A

Central

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3
Q

Branch of chemistry that deals with metals, minerals, and stuff mostly found on the periodic table.

A

Inorganic Chemistry

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4
Q

Branch of chemistry that talks about hydrocarbons and their derivatives.

A

Organic Chemistry

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5
Q

Detection and identification of substances present (qualitative analysis) or amount of each substance (quantitative analysis)

A

Analytical Chemistry

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6
Q

Branch of chemistry that deals with the processes in living organisms

A

Biochemistry

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7
Q

Branch of chemistry that covers the behavior of matter

A

Physical chemistry

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8
Q

Anything that has mass and occupies space

A

Matter

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9
Q

Measure of the quantity of matter

A

Mass

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10
Q

Amount of space

A

Volume

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11
Q

The capacity to do work or to transfer heat

A

Energy

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12
Q

Energy in motion

A

Kinetic Energy

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13
Q

Energy at rest

A

Potential Energy

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14
Q

Reaction where heat is released.

A

Exothermic

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15
Q

Reaction where heat is absorbed.

A

Endothermic

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16
Q

Ice melting is an example of ___ reaction (energy change).

A

Endothermic

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17
Q

Is energy matter?

A

No

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18
Q

State of matter that fills any container completely and highly compressible.

A

Gas

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19
Q

____ properties can be observed or measured without changing the identity of the substance.

A

Physical

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20
Q

____ properties are exhibited by matter as it undergoes changes in composition.

A

Chemical

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21
Q

Which of the following is a chemical property of matter?

A. Silver is a shiny metal that conducts electricity very well.
B. Sulfur is a yellow powder.
C. A dry piece of paper burns.
D. Pure water, for example, has a density of 0.998 g/cm^3 at 25°C.

A

C. A dry piece of paper burns.

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22
Q

___ properties are dependent on the amount of substance.

A

Extensive

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23
Q

____ properties are independent of the amount of substance.

A

Intensive

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24
Q

Which of the following is an EXTENSIVE property of matter?

A. Hardness
B. Size
C. Melting point
D. Color

A

B. Size

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25
Q

If the property is unchanged by altering the sample size, it’s an ____ property.

A

Intensive

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26
Q

A change where one or more substances are used up and one or more new substances are formed.

A

Chemical Change

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27
Q

A change where there is no change in chemical composition.

A

Physical Change

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28
Q

Which of the following exhibits a chemical change?

A. lce cream melting
B. Making a sand castle
C. A Macbook falling out of a window
D. Fireworks Exploding

A

D. Fireworks Exploding

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29
Q

TRUE OR FALSE

A physical change may suggest that a chemical change has also taken place.

A

True

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30
Q

CLASSIFICATION OF MATTER

It may be separated into pure substances by physical methods (e.g. distillation, filtration).

A

Mixture

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31
Q

CLASSIFICATION OF MATTER

It cannot be separated into simpler substances by physical methods.

A

Pure substance

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32
Q

CLASSIFICATION OF MATTER

Components are NOT distinguishable

A

Homogeneous mixtures

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33
Q

CLASSIFICATION OF MATTER

It has a fixed composition (e.g. 100% ethanol).

A

Pure substance

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34
Q

CLASSIFICATION OF MATTER

It has a single phase and the same composition throughout (i.e. same amount in any area).

A

Homogeneous mixtures

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35
Q

CLASSIFICATION OF MATTER

It has variable composition (e.g. 70%, 80%, or 95% ethanol in water).

A

Mixture

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36
Q

CLASSIFICATION OF MATTER

Preferred for drugs

A

Homogeneous mixtures

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37
Q

CLASSIFICATION OF MATTER

It does NOT have the same composition throughout (i.e. different amount in various areas) and has multiple phases.

A

Heterogeneous Mixtures

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38
Q

CLASSIFICATION OF MATTER

Components are distinguishable.

A

Heterogeneous Mixtures

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39
Q

CLASSIFICATION OF MATTER

It can be decomposed into simpler substances by chemical changes

A

Compounds

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40
Q

CLASSIFICATION OF MATTER

Water broken into hydrogen and
oxygen gases via electrolysis.

A

Compounds

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41
Q

CLASSIFICATION OF MATTER

It consists of atoms of two or more different elements bound together.

A

Compounds

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42
Q

CLASSIFICATION OF MATTER

It cannot be decomposed into simpler substance by chemical changes.

A

Elements

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43
Q

CLASSIFICATION OF MATTER

It consists of only one kind of atom.

A

Elements

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44
Q

Most abundant element in the universe

A

Hydrogen

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45
Q

The smallest unit that retains the properties of an element.

A

Atom

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46
Q

Theory that states that all matter is composed of atoms and these cannot be made or destroyed.

A

Dalton’s Theory

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47
Q

The number of protons in the nucleus of an atom that also determines its identity.

A

Atomic Number (Z)

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48
Q

The sum of the number of protons and the number of neutrons in its nucleus.

A

Mass Number (A)

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49
Q

Atoms of the same element with different
masses.

A

Isotopes

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50
Q

They are atoms containing the same number of protons but different numbers of neutrons.

A

Isotopes

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51
Q

Same mass number, different atomic numbers.

A

Isobars

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52
Q

Same number of neutrons, different atomic numbers.

53
Q

Represents the composition of the nucleus

A

Nuclide Symbol

54
Q

Formula for calculating the number of neutrons given the mass number and atomic number.

A

No.of Neutrons = Mass Number — Atomic Number

55
Q

The weighted average of the masses of an element’s isotopes.

A

Atomic Weight

56
Q

TRUE OR FALSE:

Atomic weights are fractional numbers, not integers.

57
Q

Coined the greek word “atomos” meaning uncuttable

A

Leucippus and Democritus

58
Q

Theorized atoms as solid indivisible spheres

A

Leucippus and Democritus

59
Q

Matter is made up of four elements (earth, fire, air, water).

60
Q

Atom as solid sphere but NOT indivisible.

A

John Dalton

61
Q

Who made the Solid Sphere (Billiard Ball) Model?

A

John Dalton

62
Q

Elements of a chemical compound are held together by electrical forces.

A

Humphry Davy

63
Q

Relationship between the amount of electricity used in electrolysis and the amount of chemical reaction that occurs.

A

Michael Faraday

64
Q

Coined the term “electrons” from electron ions

A

George Stoney

65
Q

Performed the Cathode-Ray Tube Experiment that provided the most convincing evidence of electrons

A

Joseph John Thomson

66
Q

Joseph John Thomson developed the ___ model of the atom.

A

Plum pudding

67
Q

The Oil-drop Experiment was performed by ___.

A

Robert Millikan

68
Q

The Oil-drop Experiment determined the charge of ___.

69
Q

Saturn-like model was made by ___.

A

Hantaro Nagaoka

70
Q

The Canal Rays Experiment was performed by ___.

A

Eugen Goldstein

71
Q

Positive rays, or positive ions, are created when the gaseous atoms in the tube lose electrons.

A

Canal Rays Experiment by Eugen Goldstein

72
Q

The Scattering Experiment was performed by ___.

A

Ernest Rutherford

73
Q

Atoms consist of very small, very dense positively charged nuclei surrounded by clouds of electrons at relatively large distances from the nuclei.

A

The Scattering Experiment by Ernest Rutherford

74
Q

Positive charge localized in the nucleus

A

Nuclear model (from The Scattering Experiment by Ernest Rutherford)

75
Q

He studied X-rays given off by various
elements.

“The number of protons in the nucleus of an atom determines its identity; this number is known as the atomic number of that element.”

A

H.G.J. Moseley

76
Q

Bombardment of beryllium with high-energy alpha-particles produced neutrons

A

J. Chadwick

77
Q

Described the electron of a hydrogen atom as revolving around its nucleus in one of a discrete set of circular orbits

A

Niels Bohr

78
Q

Proposed the idea of the wave-like nature of electrons

A

Louis de Brogli

79
Q

When an electron is excited from a lower energy level to a higher one, it absorbs a definite (quantized) amount of energy.

A

Bohr’s Planetary Model

80
Q

Quantum mechanics is based on the ___ properties of matter.

81
Q

What principle states that for electrons, it is not possible to determine the exact momentum and the exact position at the same moment in time?

A

Werner Heisenberg’s Uncertainty Principle

82
Q

It estimates the position of electrons and quantifies energy levels.

A

Erwin Schrodinger’s Wave Equation

83
Q

A region of space in which the probability of finding an electron is high.

A

Atomic Orbitals

84
Q

The Modern Atomic Model is developed by ___.

A

Erwin Schrodinger

85
Q

The Modern Atomic Model is also called ___ or ___.

A

Electron Cloud Model
Quantum Mechanical Model

86
Q

QUANTUM NUMBERS

Represents the distance of the electron from the nucleus

A

Principal QN (n)

87
Q

QUANTUM NUMBERS

Higher principal QN (n), ___ energy

88
Q

QUANTUM NUMBERS

The orbital in principal QN (n) refers to the ___ or ___.

A

Shell or energy level

89
Q

QUANTUM NUMBERS

Angular momentum QN (l) is also called ___ or ___ angular momentum QN.

A

Azimuthal or Orbital

90
Q

QUANTUM NUMBERS

The orbital in angular momentum QN (l) refers to the ___ or ___.

A

Subshell or sublevel

91
Q

QUANTUM NUMBERS

Angular momentum QN (l) is ___ less than the principal QN (n).

92
Q

QUANTUM NUMBERS

Identify the shape of the orbital based on the angular momentum QN (l).

0

A

Spherical (s-orbital)

93
Q

QUANTUM NUMBERS

Identify the shape of the orbital based on the angular momentum QN (l).

1

A

Dumb-bell (p-orbital)

94
Q

QUANTUM NUMBERS

Identify the shape of the orbital based on the angular momentum QN (l).

2

A

Cloverleaf (d-orbital)

95
Q

QUANTUM NUMBERS

Identify the shape of the orbital based on the angular momentum QN (l).

3

A

Complex (f-orbital)

96
Q

QUANTUM NUMBERS

The orbital in magnetic QN (ml) refers to the ___.

A

Specific orbital

97
Q

QUANTUM NUMBERS

It refers to the orientation in space of the orbital.

A

Magnetic QN (ml)

98
Q

QUANTUM NUMBERS

____ QN (___) is the positive and negative values of the angular momentum QN (l).

A

Magnetic QN (ml)

99
Q

QUANTUM NUMBERS

____ is used for each individual electron only.

A

Spin QN (ms)

100
Q

QUANTUM NUMBERS

Value for clockwise direction of spin

101
Q

QUANTUM NUMBERS

Value for counter-clockwise direction of spin

102
Q

This describes the distribution of electrons.

A

Electron Configuration

103
Q

It describes the number and arrangement of electrons in orbitals, subshells, and shells in an atom.

A

Electron Configuration

104
Q

Atom in its lowest energy, or unexcited, state.

A

Ground state

105
Q

What principle states that orbitals fill in order of increasing energy, from lowest to highest?

A

Aufbau principle

106
Q

No more than two electrons can occupy each orbital, and if two electrons are present, they must have opposite spins. What principle is this?

A

Pauli Exclusion Principle

107
Q

A single electron will occupy an empty orbital first before pairing.

A

Hund’s Rule

108
Q

PERIODIC TABLE OF ELEMENTS

Arranged the periodic table based on chemical properties

A

Dimitri Mendeleev

109
Q

PERIODIC TABLE OF ELEMENTS

Arranged the periodic table based on physical properties

A

Lothar Meyer

110
Q

PERIODIC TABLE OF ELEMENTS

Elements are now arranged in the periodic table in order of ___.

A

Increasing atomic number

111
Q

PERIODIC TABLE OF ELEMENTS

“The properties of the elements are periodic functions of their atomic numbers.” What do you call this law?

A

Periodic Law

112
Q

PERIODIC TABLE OF ELEMENTS

Vertical columns in the periodic table

A

Groups or families

113
Q

PERIODIC TABLE OF ELEMENTS

Horizontal rows in the periodic table

114
Q

PERIODIC TABLE OF ELEMENTS

Defined as half of the distance between the nuclei of neighboring atoms in the pure element

A

Atomic Radii (Size)

115
Q

PERIODIC TABLE OF ELEMENTS

Expressed in Angstroms (1A = 10^-10 m)

A

Atomic Radii (Size)

116
Q

PERIODIC TABLE OF ELEMENTS

The energy required to remove an electron from a gas-phase atom

A

lonization Energy (IE)

117
Q

PERIODIC TABLE OF ELEMENTS

The energy change that occurs when an electron is attached to an atom in the gas phase to form a negative ion.

A

Electron Affinity (EA)

118
Q

PERIODIC TABLE OF ELEMENTS

Measure of the relative tendency of an atom to attract electrons to itself when it is chemically combined with another atom

A

Electronegativity (EN)

119
Q

PERIODIC TABLE OF ELEMENTS

Metalloids are ___ at lower temperatures but become ___ at higher temperatures.

A

Insulators, Conductors

120
Q

PERIODIC TABLE OF ELEMENTS

Metalloids that are semiconductors

A

Silicon
Germanium
Antimony

121
Q

PERIODIC TABLE OF ELEMENTS

Non-metals are good heat ___ except carbon.

A

Insulators

122
Q

PERIODIC TABLE OF ELEMENTS

Metals have ___ electrical conductivity that ___ with increasing temperature.

A

High
Decreases

123
Q

PERIODIC TABLE OF ELEMENTS

PERIODIC TRENDS: Upper-right corner or Lower-left corner

Atomic radius

A

Lower-left corner

124
Q

PERIODIC TABLE OF ELEMENTS

PERIODIC TRENDS: Upper-right corner or Lower-left corner

Metallic character

A

Lower-left corner

125
Q

PERIODIC TABLE OF ELEMENTS

PERIODIC TRENDS: Upper-right corner or Lower-left corner

Ionization energy

A

Upper-right corner

126
Q

PERIODIC TABLE OF ELEMENTS

PERIODIC TRENDS: Upper-right corner or Lower-left corner

Electronegativity

A

Upper-right corner

127
Q

PERIODIC TABLE OF ELEMENTS

PERIODIC TRENDS: Upper-right corner or Lower-left corner

Electron affinity

A

Upper-right corner

128
Q

PERIODIC TABLE OF ELEMENTS

PERIODIC TRENDS: Upper-right corner or Lower-left corner

Non-metallic character

A

Upper-right corner

INORGANIC CHEMISTRY (5 decks)

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