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Bettelheim and Chang > Atoms > Flashcards

Atoms Flashcards

1
Q

He believed that all matter is made of very
small particles—much too small to see.

A

Democritus

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2
Q

The small particles that made up the matter is called

A

Atoms

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3
Q

Greek word of atom

A

Atomos

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4
Q

Atomos meaning

A

not to cut

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5
Q

They did not believe in atoms at all.
They insisted that matter is infinitely divisible.

A

Zeno of Elea

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6
Q

It is a substance (for example, carbon, hydrogen, and iron) that
consists of identical atoms.

A

Element

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7
Q

Number of elements occur in nature

A

88

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8
Q

It is a pure substance made up of two or more elements in a
fixed ratio by mass.

A

Compound

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9
Q

The big four elements

A

Carbon, Hydrogen, Oxygen, Nitrogen

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10
Q

It is a pure substance made up of two or more elements in a
fixed ratio by mass.

A

mixture

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11
Q

All matter is made up of very tiny, indivisible particles, which Dalton
called

A

atoms

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12
Q

is a tightly bound combination of two or more atoms that
acts as a single unit.

A

Molecule

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13
Q

He discovered the law of conservation of mass

A

Antoine Laurent Lavoisier

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14
Q

states that matter can be
neither created nor destroyed.

A

law of conservation of mass

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15
Q

which states that any compound is always
made up of elements in the same proportion by mass.

A

law of constant composition

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16
Q

He discovered the law of constant composition

A

Joseph Proust

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17
Q

consist of single atoms
that are not connected to each other

A

Monoatomic elements

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18
Q

Example of monoatomic elements

A

Helium and Neon

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19
Q

contains two atoms in
each molecule, connected to each other by a chemical bond.

A

Diatomic elements

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20
Q

Example of diatomic elements

A

H, N, F, Cl, Br, and I

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21
Q

Some elements have even more atoms in each molecule.

A

Polyatomic elements

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22
Q

Are referred to as polyatomic elements.

A

Diamond and S8

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23
Q

A subatomic particle with
a charge of 11 and a mass of
approximately 1 amu; it is found
in a nucleus.

A

Proton

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24
Q

A unit
of the scale of relative masses of
atoms: 1 amu = 1.6605x10^-24 g

A

Atomic mass unit

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25
Q

A subatomic particle
with a charge of 21 and a mass
of approximately 0.0005 amu. It is
found in the space surrounding a
nucleus.

A

Electron

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26
Q

A subatomic particle
with a mass of approximately
1 amu, and a charge of zero; it is found in the nucleus

A

Neutron

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27
Q

which is the sum of the number
of protons and neutrons in its nucleus.

A

Mass number

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28
Q

It is the number of protons in its nucleus.

A

Atomic number

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29
Q

Atoms with the same number of protons but
different numbers of neutrons are called

A

Isotopes

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30
Q

It is a weighted average of the masses (in amu) of its isotopes found on the Earth.

A

Atomic weight

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31
Q

A typical heavy atom (although not the heaviest) is

A

Lead-208

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32
Q

He produced one of the first periodic tables, the form of which we
still use today

A

Dmitri Mendeleev

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33
Q

Horizontal rows of periodic table

A

Periods

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34
Q

Vertical columns of periodic table

A

Groups

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35
Q

Chlorine, Bromine, Iodine

A

Halogens

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36
Q

They are solids (except for mercury, which is a liquid), shiny, conductors of electricity, ductile (they can be drawn into wires), and malleable (they can be hammered and rolled into sheets).

A

Metals

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37
Q

Second class of elements

A

Nonmetals

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38
Q

These elements have some properties of
metals and some properties of nonmetals.

A

Metalloids

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39
Q

He said that only certain values of kinetic energy of electrons are possible (energy levels); values in between are not permitted

A

Neils Bohr

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40
Q

He said that electrons in atoms do not move freely in space around nucleus; confined to specific regions called principal energy levels/ shells

A

Neils Bohr

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41
Q

The lowest possible energy
level is the

A

Ground state

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42
Q

electrons in atoms do not move freely in the space around the nucleus, but rather are confined to specific regions of space called

A

Principal energy level = shells

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43
Q

Shells are divided into

A

Subshells

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44
Q

region of space and can hold two electrons

A

orbitals

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45
Q

is a description of the orbitals that
its electrons occupy.

A

Electron configuration

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46
Q

Outer-shell electrons are
called

A

Valence electrons

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47
Q

energy level in which valence electrons are found is
called the

A

Valence shell

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48
Q

To show the outermost electrons of an atom, we commonly use a representation called

A

Lewis dot structure

49
Q

Lewis dot structure is named after

A

Gilbert N. Lewis

50
Q

It shows the symbol of the element surrounded by a number of dots equal to
the number of electrons in the outer shell of an atom of that element.

A

Lewis Structure

51
Q

It is a measure of how difficult it is to remove the
most loosely held electron from an atom in the gaseous state.

A

Ionization energy

52
Q

It involves only the separation, combination, or rearrangement
of atoms; it does not result in their creation or destruction.

A

Chemical reaction

53
Q

States that different samples of the
same compound always contain its constituent elements in the same proportion by mass

A

Law of definite proportions

54
Q

if two elements can combine to form more than one und, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers

A

Law of multiple proportions

55
Q

the emission and transmission of energy through space in the form of waves.

A

Radiation

56
Q

Negatively charged plate

A

Cathode

57
Q

positively charged plate

A

Anode

58
Q

He noticed that cathode rays caused glass
and metals to emit very unusual rays.

A

Wilhelm Roentgen

59
Q

He found that exposing thickly wrapped photographic plates to a certain uranium compound caused them to darken, even without the stimulation of cathode rays

A

Antoine Becquerel

60
Q

spontaneous emission of particles and/or radiation

A

Radioactivity

61
Q

spontaneous emission of particles and/or radiation

A

Radioactive

62
Q

Suggested the name radioactivity

A

Marie Curie

63
Q

consist of positively charged particles

A

Alpha particles

64
Q

electrons and are deflected by the negatively charged plate

A

Beta particles

65
Q

type of radioactive radiation consists of high-energy rays called

A

Gamma rays

66
Q

He determined the charge of electron

A

Robert Andrews Millikan

67
Q

He investigated the structure of the
atomic nucleus.

A

Ernest Rutherford

68
Q

HE focused on the structure of the atomic nucleus and on radioactivity.

A

Johannes Hans Wilhelm Geiger

69
Q

A device for measuring radiation that is now commonly called the

A

Geiger counter

70
Q

He proved the existence
of neutrons

A

James Chadwick

71
Q

an ion with a net positive charge

A

Cation

72
Q

an ion whose net charge is negative due to an increase in the number of electrons.

A

Anion

73
Q

It is formed from cations and anions

A

Ionic compound

74
Q

Used to express the composition of molecules and ionic compounds in terms of chemical symbols.

A

Chemical formulas

75
Q

shows the exact number of atoms of each element in the smallest unit of a substance

A

Molecular formula

76
Q

one of two or more distinct forms of an element.

A

Allotrope

77
Q

It tells us which elements are present and the simplest whole-number ratio of their atoms

A

Empirical formula

78
Q

compounds formed from just
two elements.

A

Binary compounds

79
Q

compounds consisting of three elements.

A

Tertiary compounds

80
Q

can be described as a substance that yields hydrogen ions (H+) when dissolved
in water.

A

Acid

81
Q

are acids that contain hydrogen, oxygen, and another element (the central element). T

A

Oxoacids

82
Q

can be described as a substance that yields hydroxide ions (OH-) when dissolved in water

A

Base

83
Q

discovered that atoms and molecules emit energy only in certain discrete quantities, or quanta

A

Max Planck

84
Q

a vibrating disturbance by which energy is transmitted

A

wave

85
Q

the distance between identical points on successive waves

A

wavelength

86
Q

number of waves that pass through a particular point in one second

A

frequency

87
Q

vertical distance from the midline of a wave to the peak or trough.

A

amplitude

88
Q

proposed that visible light consists of electromagnetic waves

A

James Maxwell

89
Q

has an electric field component and a magnetic field component

A

electromagnetic wave

90
Q

the emission and transmission of energy in the form of electromagnetic waves

A

electromagnetic radiation

91
Q

the smallest quantity of energy that can be
emitted (or absorbed) in the form of electromagnetic radiation

A

quantum

92
Q

the smallest quantity of energy that can be
emitted (or absorbed) in the form of electromagnetic radiation.

A

photoelectric effect

93
Q

photoelectric effect is also called

A

threshold frequency

94
Q

particles of light

A

photons

95
Q

either continuous or line spectra of radiation emitted by substances

A

emission spectra

96
Q

the light emission only at specific wavelengths

A

line spectra

97
Q

the lowest energy state of a system

A

ground state

98
Q

higher in energy than the ground state

A

excited state

99
Q

he proposed that matter and radiation have the properties of both wave and particle

A

Louis de Broglie

100
Q

it is impossible to know simultaneously both the momentum p (defined as mass times velocity) and the position of a particle with certainty

A

Heisenberg uncertainty principle

101
Q

specifies the possible energy states the electron can occupy in a hydrogen atom and identifies the corresponding wave functions

A

Schrodinger equation

102
Q

gives the probability that an electron will be found in a particular region of an atom

A

electron density

103
Q

the wave function of an electron in an atom

A

atomic orbital

104
Q

describe the distribution of electrons in hydrogen and other atom

A

quantum numbers

105
Q

determines the energy of an orbital

A

principal quantum number

106
Q

tells us the “shape” of the orbitals

A

angular momentum quantum number

107
Q

A collection of orbitals with the same value of n is frequently called a

A

shell

108
Q

describes the orientation of the orbital in space

A

magnetic quantum number

109
Q

To take the electron spin into account, it is necessary to introduce a fourth quantum number

A

electron spin quantum number

110
Q

encloses about 90 percent of the total electron density in an orbital

A

boundary surface diagram

111
Q

encloses about 90 percent of the total electron density in an orbital

A

electron configuration

112
Q

no two electrons in an atom can have the same
four quantum numbers

A

Pauli exclusion principle

113
Q

are attracted by a magnet

A

Paramagnetic substances

114
Q

are slightly repelled by a magnet

A

Diamagnetic

115
Q

the most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins

A

Hund’s rule

116
Q

as protons are added one by one to the nucleus to build up the elements, electrons are similarly added to the atomic orbitals

A

Aufbau principle

117
Q

the minimum energy (in kJ/mol) required to remove an electron from a gaseous atom in its ground state

A

Ionization energy

118
Q

the radius of a cation or an anion

A

Ionic radius

119
Q

the energy change that occurs when an electron is accepted by an atom in the gaseous
state to form an anion

A

Electron affinity

Bettelheim and Chang (7 decks)

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