Chemistry 1124 Flashcards
1
Q
a pattern of regularly recurring properties
A
periodicity
2
Q
the number of protons in the nucleus of each atom
A
atomic number
3
Q
the vertical columns of the Periodic Table of the Elements
A
groups
4
Q
the horizontal rows of the Periodic Table of Elements
A
periods
5
Q
a set of elements with similar properties
A
family
6
Q
the most chemically active metals
A
alkali metals
7
Q
the most reactive nonmetals
A
halogens
8
Q
the least reactive elements
A
noble gases
9
Q
a complete s and p sublevel in the highest occupied energy level
A
stable octet
10
Q
the s-block elements in Group IA
A
alkali metal
11
Q
very reactive Group VIIA nonmetals with one electron short of a stable octet
A
halogens
12
Q
the elements in Groups IIIB through IIB, also called d-block elements
A
transition metals
13
Q
Group VIIIA elements with a stable octet or duet
A
noble gases
14
Q
the s-block elements in Group IIA
A
alkaline earth metals
15
Q
elements with both metal and nonmetal properties, also called semimetals
A
metalloid
16
Q
NAME
published first Periodic Table of Elements
A
Dmitri Mendeleev
17
Q
NAME
location of the First International Congress of Chemists
A
Karlsruhe, Germany
18
Q
NAME
proposed the law of octaves
A
John Newlands
19
Q
NAME
organized elements into triads
A
Johann Dobereiner
20
Q
NAME
presented a new method for determining atomic masses
A
Stanislao Canizzaro
21
Q
NAME
determined positive charge of atom
A
Henry Moseley
22
Q
_____ are the electrons in the outermost energy level and are responsible for the ____ of an element
A
Valence electrons; physical properties
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
24
Q
The metalloids include the elements boron, silicon, ____, arsenic, selenium, antimony, and ____
A
germanium; tellurium
25
Henry Moseley used x-ray diffraction to determine the amount of ______ in the nucleus of each atom
positive charge
26
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
mass; number
27
No two electrons in the same atom can have the same four quantum numbers
Pauli exclusion principle
28
An electron occupies the lowest energy orbital that can receive it
Aufbau principle
29
The orbitals of equal energy are each occupied by one electron
Hund's rule
30
The physical and chemical properties of the elements are periodic functions of their atomic numbers
periodic law
31
____ electrons in the outermost energy level are responsible for the properties of an element`
Valence
32
A ______ consists of eight electrons-a complete s and d p sublevel- in the highest occupied energy level
stable octet
33
one half the distance from the nucleus of one atom to the nucleus of an adjacent, identical atom in a molecule
atomic radius
34
any process that results in the formation of an ion
ionization
35
the energy required to cause a gaseous atom or ion to release an electron
ionization energy
36
the amount of energy involved when an electron acquired by a neutral gaseous atom
electron affinity
37
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
chemical formula
38
the distance that which attraction is greatest and potential energy is least
bond length
39
a covalent bond in which the bonding electrons are shared equally by both atoms
nonpolar
40
a covalent bond in which the bonding electrons are shared unequally by both atoms
polar
41
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
octet rule
42
all objects within a closed system tend to move toward a state of greater stability but lower potential energy
second law of thermodynamics
43
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
periodic function
44
the measure of the power of an atom in a molecule to attract electrons to itself
electronegativity
45
an energy required to dislodge a (second) electron form an atom or ion
(second) ionization energy
46
____ is generally determined by how easily an atom gives up an electron or by how closely an element resembles ______
Metallic character; the physical properties of a metal
47
If an atom gains an electron and achieves a ____ stable electron structure, energy is released
more
48
If an atom gains an electron and achieves a ____ stable electron structure, energy is gained
less
49
An electron affinity with a ____ value indicates an endothermic reaction; a ____ value indicates an exothermic reaction
positive; negative
50
Electronegativity values are based on the electronegativity of the element ____
fluorine
51
The three types of chemical bonds are ____ bonds, ____ bonds, and ____ bonds
covalent; ionic; metallic
52
attractive force that holds atoms together in compounds
chemical bond
53
energy required to break a chemical bond
bond energy
54
bond created by attraction of ions
ionic bond
55
bond created by sharing of electrons
covalent bond
56
bond formed with metal ions and free electrons
metallic bond
57
molecule containing only two atoms
diatomic molecule
58
simplest unit indicated by the formula of any compound
formula unit
59
shows the types and numbers of atoms in a single molecule
molecular formula
60
pair of electrons that enters into the covalent bond
shared pair
61
pair of electrons that does not enter into the covalent bond
unshared pair
62
ion with a positive charge
cation
63
ion with a negative charge
anion
64
The formation of a chemical bond is an ____ reaction--energy is released
exothermic
65
Breaking a chemical bond is an ____ reaction--additional energy is required
endothermic
66
a substance consisting of atoms joined by covalent bonds into a crystalline structure
network covalent substance
67
electrostatic repulsion between the valence level electron pairs surrounding an atom causes these pairs to be oriented as far apart as possible
VSEPR
68
a large crystal formed by a network covalent structure
macromolecules
69
the combining of atomic orbitals of similar energies on the same atom to provide special orbitals of equal energy for the purpose of bonding
hybridization
70
a covalently bonded group of atoms with an overall positive or negative charge
polyatomic ion
71
intermolecular forces stronger than dipole-dipole forces
hydrogen bonds
72
collective name for all intermolecular forces
Van Der Waals forces
73
any bonding situation that cannot be properly represented by a single Lewis structure
Resonance
74
forces of attraction between dipoles of polar covalent molecules
dipole-dipole forces
75
the intermolecular attractions resulting from electron motion and the creation of instantaneous, induced dipoles
London dispersion forces
76
clouds of delocalized mobile electrons
electron sea
77
bond between cations and anions
ionic bond
78
permanent change in shape
deformation
79
ionic character less than 5% (electronegativity difference less than 0.3)
nonpolar covalent
80
bond between positive metal ions and mobile electrons
metallic bond
81
Because of their _____, network covalent substances are very hard and have high melting temperatures
crystalline structure
82
______ are large crystals formed by network covalent substances
Macromolecules
83
The ____ theory and the ____ theory are two theories used to predict molecular shape
VSEPR; hybridization
84
The geometric shape of a molecule is determined by the number of ____, the ____ pairs of electrons, and the ____ of the atoms
atoms; unshared; partial charge
85
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; B; E
86
Most ____ compounds have crystalline structures consisting of small formula units that bond together to form the three-dimensional structure of the ____
ionic; crystal
87
Of those two types of bonds, covalent and ionic, the ____ is the stronger bond
ionic
88
Metals are good conductors of electricity because the electric charge is transferred by the ____
mobile electrons
89
Ionic character is determined by the difference between the ______ of the two bonding elements
electronegativities
90
Three types of intermolecular forces are ____ forces, ____ bonds, and ____ forces
dipole-dipole; hydrogen; London dispersion
91
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
hydrogen bond
92
The ____ bonds between water molecules account for the high heat of vaporization of water
hydrogen
93
bond between cations and anion
ionic bonds
94
The comparative strength of ionic bonds accounts for the ____, ____, and high melting temperatures of ionic compounds
hardness; strength
95
When individual atoms or ions bond and achieve a _____, energy is released and the atoms move into a state of ____
stable octet; lower potential energy
