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chemistry 12 > ATOMIC THEORY chapter 3/4 > Flashcards

ATOMIC THEORY chapter 3/4 Flashcards

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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
Q

trigonal bipyramidal

A

5 electron pairs
no lone pairs
90, 180 degree

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26
Q

octahedral

A

6 electron pairs
no lone pairs
90 degree

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27
Q

trigonal planar

A

3 electron pairs
no lone pairs
120 degree

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28
Q

intramolecular bond

A

the chemical bond within a molecule

29
Q

intermolecular force

A

a force that causes one molecule to interact with another molecule; occurs between molecules

30
Q

van der Waals forces

A

many types of
intermolecular forces, including dipole–
dipole forces, London dispersion forces,
and hydrogen bonding

31
Q

dipole-dipole force

A

the intermolecular
force that is caused when the dipoles of
polar molecules position their positive and
negative ends near each other

32
Q

hydrogen bond

A

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
Q

London dispersion forces

A

the intermolecular forces that exist in nonpolar molecules; they increase as the
molecular mass increases

34
Q

polarizability

A

the ability of a substance to
form a dipolar charge distribution

35
Q

surface tension

A

the resistance of a liquid
to increase its surface area

36
Q

capillary action

A

the spontaneous rising
of a liquid in a narrow tube

37
Q

viscosity

A

the measure of a liquid’s
resistance to flow

38
Q

composite material

A

a material composed
of two or more distinct materials that
remain separate from each other in the
solid phase

39
Q

metallic crystal

A

a solid with closely
packed atoms held together by electrostatic
interactions and free-moving electrons

40
Q

electron sea theory

A

a theory that states
that the electrons in a metallic crystal
move freely around the positively charged
nuclei

41
Q

metallic bonding

A

the bonding that holds the nuclei and electrons of metals together

42
Q

molecular crystal

A

a solid composed
of individual molecules held together by
intermolecular forces of attraction

43
Q

buckyball

A

a spherical arrangement of
carbon atoms that forms a hollow,
cage-like structure

44
Q

carbon nanotube

A

a solid made of carbon atoms similar to graphite rolled into a cylinder

45
Q

semi conductor

A

a substance that
conducts a slight electric current at
room temperature but has increasing
conductivity at higher temperatures

46
Q

ionic metal properties

A

High melting point*

Low vapor pressure*

Nonconductors of
electricity*

Brittle*

47
Q

molecular metal properties

A

Low melting point*

Do not conduct
electricity*

48
Q

metallic metal properties

A

Good conductor of
heat/electricity*

Malleable/Ductile*

49
Q

network metal properties

A

High melting point*

Hard*

50
Q

J.J. Thomason discovery

A

electron through cathode ray experiment

51
Q

Millikan discovery

A

charge of electron through charged oil drop experiment

52
Q

Rutherford discovery

A

nucleus and protons through gold foil experiment

53
Q

radioactivity

A

spontaneous decay or disintegration of an atom

54
Q

isotope

A

atoms with the same number of protons but different numbers of neutrons

55
Q

atomic number

A

number of protons in a nucleus

56
Q

mass number

A

total number of protons and neutrons in a nucleus

57
Q

radioisoptope

A

an isotope that emits radioactive gamma rays and/or subatomic particles (alpha and/or beta particles)

58
Q

photoelectric effect

A

electrons are emitted by matter that absorbs energy from shortwave electromagnetic radiation (for example, visible or UV light)

59
Q

Planck’s discovery

A

quantum theory

60
Q

quantum

A

a unit or packet of energy

61
Q

photon

A

unit of light energy

62
Q

Einstein discovered

A

photoelectric effect (explanation) and photons

63
Q

Bohr discovered

A

electron energy levels

64
Q

quantum numbers

A

1 (n) - energy level/shell
2 (l) - shape spdfg
3 (ml) - magnetic quantum number, orientation
4 (ms) - spin quantum number

65
Q

aufbau principle

A

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
Q

electron configuration

A

the location and number of electrons in the electron energy levels of an atom

67
Q

energy-level diagram

A

a diagram that represents the relative energies
of the electrons in an atom

68
Q

Hund’s rule

A

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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