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chemistry 12 > ATOMIC THEORY chapter 3/4 > Flashcards

ATOMIC THEORY chapter 3/4 Flashcards

(68 cards)

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1
Q

ionic bond

A

the electrostatic attraction
between oppositely charged ions

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2
Q

isoelectronic

A

having the same number of
electrons per atom, ion, or molecule

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3
Q

covalent bond

A

a chemical bond in which
atoms share the bonding electrons

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4
Q

bonding electron pair

A

an electron pair that is involved in bonding, found in the space between 2 atoms

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5
Q

lewis structure

A

a diagram that
represents the arrangement of covalent
electrons and bonds in a molecule or
polyatomic ion

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6
Q

duet rule

A

the observation that the
complete outer shell of valence electrons
when hydrogen and period 2 metals are
involved in bonding

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7
Q

octet rule

A

the observation that many
atoms tend to form the most stable
substances when they are surrounded by
8 electrons in their valence shells

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8
Q

lone electron pair

A

a pair of valence electrons that is localized to a given atom but not involved in bonding

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9
Q

simplified lewis structure

A

a Lewis structure in which bonding electron pairs are represented by solid lines and lone
electron pairs by dots

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10
Q

space-filling model

A

a model of a molecule showing the relative sizes of the atoms and their relative orientations

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11
Q

coordinate covalent bond

A

a model of a molecule showing the relative sizes of the atoms and their relative orientations

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12
Q

three-dimensional structure

A

the three dimensional arrangement of ions or atoms making up a pure substance

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13
Q

valence shell electron-pair repulsion
(VSEPR) theory

A

a method to determine
the geometry of a molecule based on the
idea that electron pairs are as far apart as
possible

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14
Q

electron-pair repulsion

A

the repulsive force that occurs between electron pairs, causing them to be positioned as far apart as possible in a molecule

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15
Q

most common/need to know structures

A

linear 180
trigonal planar 120
tetrahedral 109.5
trigonal bipyramidal 90, 120
octahedral 90

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16
Q

non-polar covalent bond

A

a covalent bond in which the electrons are shared equally between atoms

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17
Q

polar covalent bond

A

a covalent bond in
which the electrons are not shared equally
because 1 atom attracts them more
strongly than the other atom

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18
Q

electronegativity

A

the ability of an atom
in a molecule to attract shared electrons
to itself

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19
Q

dipole

A

a separation of positive and 
negative charges in a region in space

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20
Q

polar molecule

A

a molecule that has a net
dipole

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21
Q

non-polar molecule

A

a molecule that has
only non-polar bonds, or a bond dipole
sum of zero

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22
Q

trigonal planar

A

3 electron pairs
no lone pairs
120 degree

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23
Q

linear

A

2 electron pairs
no lone pairs
180 degree

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24
Q

tetrahedral

A

4 electron pairs
no lone pairs
109.5 degree

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25
trigonal bipyramidal
5 electron pairs no lone pairs 90, 180 degree
26
octahedral
6 electron pairs no lone pairs 90 degree
27
trigonal planar
3 electron pairs no lone pairs 120 degree
28
intramolecular bond
the chemical bond within a molecule
29
intermolecular force
a force that causes one molecule to interact with another molecule; occurs between molecules
30
van der Waals forces
many types of intermolecular forces, including dipole– dipole forces, London dispersion forces, and hydrogen bonding
31
dipole-dipole force
the intermolecular force that is caused when the dipoles of polar molecules position their positive and negative ends near each other
32
hydrogen bond
the strong dipole–dipole force that occurs when a hydrogen atom bonded to a highly electronegative atom (oxygen, nitrogen, or fluorine) is attracted to a partially negative atom on a nearby molecule
33
London dispersion forces
the intermolecular forces that exist in nonpolar molecules; they increase as the molecular mass increases
34
polarizability
the ability of a substance to form a dipolar charge distribution
35
surface tension
the resistance of a liquid to increase its surface area
36
capillary action
the spontaneous rising of a liquid in a narrow tube
37
viscosity
the measure of a liquid’s resistance to flow
38
composite material
a material composed of two or more distinct materials that remain separate from each other in the solid phase
39
metallic crystal
a solid with closely packed atoms held together by electrostatic interactions and free-moving electrons
40
electron sea theory
a theory that states that the electrons in a metallic crystal move freely around the positively charged nuclei
41
metallic bonding
the bonding that holds the nuclei and electrons of metals together
42
molecular crystal
a solid composed of individual molecules held together by intermolecular forces of attraction
43
buckyball
a spherical arrangement of carbon atoms that forms a hollow, cage-like structure
44
carbon nanotube
a solid made of carbon atoms similar to graphite rolled into a cylinder
45
semi conductor
a substance that conducts a slight electric current at room temperature but has increasing conductivity at higher temperatures
46
ionic metal properties
High melting point* Low vapor pressure* Nonconductors of electricity* Brittle*
47
molecular metal properties
Low melting point* Do not conduct electricity*
48
metallic metal properties
Good conductor of heat/electricity* Malleable/Ductile*
49
network metal properties
High melting point* Hard*
50
J.J. Thomason discovery
electron through cathode ray experiment
51
Millikan discovery
charge of electron through charged oil drop experiment
52
Rutherford discovery
nucleus and protons through gold foil experiment
53
radioactivity
spontaneous decay or disintegration of an atom
54
isotope
atoms with the same number of protons but different numbers of neutrons
55
atomic number
number of protons in a nucleus
56
mass number
total number of protons and neutrons in a nucleus
57
radioisoptope
an isotope that emits radioactive gamma rays and/or subatomic particles (alpha and/or beta particles)
58
photoelectric effect
electrons are emitted by matter that absorbs energy from shortwave electromagnetic radiation (for example, visible or UV light)
59
Planck's discovery
quantum theory
60
quantum
a unit or packet of energy
61
photon
unit of light energy
62
Einstein discovered
photoelectric effect (explanation) and photons
63
Bohr discovered
electron energy levels
64
quantum numbers
1 (n) - energy level/shell 2 (l) - shape spdfg 3 (ml) - magnetic quantum number, orientation 4 (ms) - spin quantum number
65
aufbau principle
the theory that an atom is “built up” by the addition of electrons, which fill orbitals starting at the lowest available energy orbital before filling higher energy orbitals (for example, 1s before 2s)
66
electron configuration
the location and number of electrons in the electron energy levels of an atom
67
energy-level diagram
a diagram that represents the relative energies of the electrons in an atom
68
Hund's rule
a rule stating that in a particular set of orbitals of the same energy, the lowest energy configuration for an atom is the one with the maximum number of unpaired electrons allowed by the Pauli exclusion principle; unpaired electrons are represented as having parallel spins

chemistry 12 (5 decks)

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