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Chemistry 1124 Flashcards

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1
Q

a pattern of regularly recurring properties

A

periodicity

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2
Q

the number of protons in the nucleus of each atom

A

atomic number

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3
Q

the vertical columns of the Periodic Table of the Elements

A

groups

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4
Q

the horizontal rows of the Periodic Table of Elements

A

periods

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5
Q

a set of elements with similar properties

A

family

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6
Q

the most chemically active metals

A

alkali metals

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7
Q

the most reactive nonmetals

A

halogens

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8
Q

the least reactive elements

A

noble gases

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9
Q

a complete s and p sublevel in the highest occupied energy level

A

stable octet

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10
Q

the s-block elements in Group IA

A

alkali metal

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11
Q

very reactive Group VIIA nonmetals with one electron short of a stable octet

A

halogens

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12
Q

the elements in Groups IIIB through IIB, also called d-block elements

A

transition metals

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13
Q

Group VIIIA elements with a stable octet or duet

A

noble gases

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14
Q

the s-block elements in Group IIA

A

alkaline earth metals

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15
Q

elements with both metal and nonmetal properties, also called semimetals

A

metalloid

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16
Q

NAME

published first Periodic Table of Elements

A

Dmitri Mendeleev

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17
Q

NAME

location of the First International Congress of Chemists

A

Karlsruhe, Germany

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18
Q

NAME

proposed the law of octaves

A

John Newlands

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19
Q

NAME

organized elements into triads

A

Johann Dobereiner

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20
Q

NAME

presented a new method for determining atomic masses

A

Stanislao Canizzaro

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21
Q

NAME

determined positive charge of atom

A

Henry Moseley

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22
Q

_____ are the electrons in the outermost energy level and are responsible for the ____ of an element

A

Valence electrons; physical properties

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23
Q

Inner electrons do not have a great effect on chemical properties because the rarely _____

A

come into contact with the atom’s environment

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24
Q

The metalloids include the elements boron, silicon, ____, arsenic, selenium, antimony, and ____

A

germanium; tellurium

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25
Q

Henry Moseley used x-ray diffraction to determine the amount of ______ in the nucleus of each atom

A

positive charge

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26
Q

Mendeleev based his Periodic Table of the Elements on the atomic ____ of each element, but the modern Periodic Table is based on the atomic ____ of each element

A

mass; number

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27
Q

No two electrons in the same atom can have the same four quantum numbers

A

Pauli exclusion principle

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28
Q

An electron occupies the lowest energy orbital that can receive it

A

Aufbau principle

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29
Q

The orbitals of equal energy are each occupied by one electron

A

Hund’s rule

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30
Q

The physical and chemical properties of the elements are periodic functions of their atomic numbers

A

periodic law

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31
Q

____ electrons in the outermost energy level are responsible for the properties of an element`

A

Valence

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32
Q

A ______ consists of eight electrons-a complete s and d p sublevel- in the highest occupied energy level

A

stable octet

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33
Q

one half the distance from the nucleus of one atom to the nucleus of an adjacent, identical atom in a molecule

A

atomic radius

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34
Q

any process that results in the formation of an ion

A

ionization

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35
Q

the energy required to cause a gaseous atom or ion to release an electron

A

ionization energy

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36
Q

the amount of energy involved when an electron acquired by a neutral gaseous atom

A

electron affinity

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37
Q

a symbolic representation of the composition of a compound using elemental symbols and numerical subscripts to show both the kinds of elements that compose the compound and the proportion of atoms of each element in the compound

A

chemical formula

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38
Q

the distance that which attraction is greatest and potential energy is least

A

bond length

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39
Q

a covalent bond in which the bonding electrons are shared equally by both atoms

A

nonpolar

40
Q

a covalent bond in which the bonding electrons are shared unequally by both atoms

A

polar

41
Q

elements tend to react chemically to form compounds so that each atom, by gaining, losing, or sharing electrons, achieves a stable octet in its highest occupied energy level

A

octet rule

42
Q

all objects within a closed system tend to move toward a state of greater stability but lower potential energy

A

second law of thermodynamics

43
Q

any property of an element that increases or decreases in character or intensity as the atomic number increases, either along a period or down a group in the Periodic Table of Elements

A

periodic function

44
Q

the measure of the power of an atom in a molecule to attract electrons to itself

A

electronegativity

45
Q

an energy required to dislodge a (second) electron form an atom or ion

A

(second) ionization energy

46
Q

____ is generally determined by how easily an atom gives up an electron or by how closely an element resembles ______

A

Metallic character; the physical properties of a metal

47
Q

If an atom gains an electron and achieves a ____ stable electron structure, energy is released

A

more

48
Q

If an atom gains an electron and achieves a ____ stable electron structure, energy is gained

A

less

49
Q

An electron affinity with a ____ value indicates an endothermic reaction; a ____ value indicates an exothermic reaction

A

positive; negative

50
Q

Electronegativity values are based on the electronegativity of the element ____

A

fluorine

51
Q

The three types of chemical bonds are ____ bonds, ____ bonds, and ____ bonds

A

covalent; ionic; metallic

52
Q

attractive force that holds atoms together in compounds

A

chemical bond

53
Q

energy required to break a chemical bond

A

bond energy

54
Q

bond created by attraction of ions

A

ionic bond

55
Q

bond created by sharing of electrons

A

covalent bond

56
Q

bond formed with metal ions and free electrons

A

metallic bond

57
Q

molecule containing only two atoms

A

diatomic molecule

58
Q

simplest unit indicated by the formula of any compound

A

formula unit

59
Q

shows the types and numbers of atoms in a single molecule

A

molecular formula

60
Q

pair of electrons that enters into the covalent bond

A

shared pair

61
Q

pair of electrons that does not enter into the covalent bond

A

unshared pair

62
Q

ion with a positive charge

A

cation

63
Q

ion with a negative charge

A

anion

64
Q

The formation of a chemical bond is an ____ reaction–energy is released

A

exothermic

65
Q

Breaking a chemical bond is an ____ reaction–additional energy is required

A

endothermic

66
Q

a substance consisting of atoms joined by covalent bonds into a crystalline structure

A

network covalent substance

67
Q

electrostatic repulsion between the valence level electron pairs surrounding an atom causes these pairs to be oriented as far apart as possible

A

VSEPR

68
Q

a large crystal formed by a network covalent structure

A

macromolecules

69
Q

the combining of atomic orbitals of similar energies on the same atom to provide special orbitals of equal energy for the purpose of bonding

A

hybridization

70
Q

a covalently bonded group of atoms with an overall positive or negative charge

A

polyatomic ion

71
Q

intermolecular forces stronger than dipole-dipole forces

A

hydrogen bonds

72
Q

collective name for all intermolecular forces

A

Van Der Waals forces

73
Q

any bonding situation that cannot be properly represented by a single Lewis structure

A

Resonance

74
Q

forces of attraction between dipoles of polar covalent molecules

A

dipole-dipole forces

75
Q

the intermolecular attractions resulting from electron motion and the creation of instantaneous, induced dipoles

A

London dispersion forces

76
Q

clouds of delocalized mobile electrons

A

electron sea

77
Q

bond between cations and anions

A

ionic bond

78
Q

permanent change in shape

A

deformation

79
Q

ionic character less than 5% (electronegativity difference less than 0.3)

A

nonpolar covalent

80
Q

bond between positive metal ions and mobile electrons

A

metallic bond

81
Q

Because of their _____, network covalent substances are very hard and have high melting temperatures

A

crystalline structure

82
Q

______ are large crystals formed by network covalent substances

A

Macromolecules

83
Q

The ____ theory and the ____ theory are two theories used to predict molecular shape

A

VSEPR; hybridization

84
Q

The geometric shape of a molecule is determined by the number of ____, the ____ pairs of electrons, and the ____ of the atoms

A

atoms; unshared; partial charge

85
Q

According to the shape notation of the VSEPR, the central atom is indicated with the letter __, the number of atoms surrounding the central atom is indicated with the letter __ and a subscript, and the number of unshred pairs of electrons is indicated by the letter __ with subscripts

A

A; B; E

86
Q

Most ____ compounds have crystalline structures consisting of small formula units that bond together to form the three-dimensional structure of the ____

A

ionic; crystal

87
Q

Of those two types of bonds, covalent and ionic, the ____ is the stronger bond

A

ionic

88
Q

Metals are good conductors of electricity because the electric charge is transferred by the ____

A

mobile electrons

89
Q

Ionic character is determined by the difference between the ______ of the two bonding elements

A

electronegativities

90
Q

Three types of intermolecular forces are ____ forces, ____ bonds, and ____ forces

A

dipole-dipole; hydrogen; London dispersion

91
Q

the intermolecular attraction between a hydrogen atom bonded to a strongly electronegative atom and an unshared pair of electrons on a strongly electronegative atom of another molecule

A

hydrogen bond

92
Q

The ____ bonds between water molecules account for the high heat of vaporization of water

A

hydrogen

93
Q

bond between cations and anion

A

ionic bonds

94
Q

The comparative strength of ionic bonds accounts for the ____, ____, and high melting temperatures of ionic compounds

A

hardness; strength

95
Q

When individual atoms or ions bond and achieve a _____, energy is released and the atoms move into a state of ____

A

stable octet; lower potential energy

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