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chem > DAT Gen Chem Atomic and Molecular structure > Flashcards

DAT Gen Chem Atomic and Molecular structure Flashcards

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1
Q

are closest to
the positively charged nucleus.

A

core electrons

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2
Q

which electrons are the most stable and are lowest in energy.

A

core electrons

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3
Q

Changing the number of neutrons of an atom, leaving protons the same

A

isotope

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4
Q

what produces ions

A

changing the number of electrons

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5
Q

elements within a compound always combine in
a fixed proportion.

A

law of constant composition

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6
Q

the molecules undergo
rearrangement to produce a physical change.

A

physical reaction

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7
Q

involve
the substances undergoing a chemical change
whereby a new substance is created.

A

chemical reaction

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8
Q

when two or
more atoms or molecules combine to form
a single compound.

A

synthesis rxn

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9
Q

when a
compound breaks down into two or more
products.

A

decomposition rxn

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10
Q

when
one element is replaced by another in a
compound.

A

single displacement rxn

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11
Q

exchange
of bonds between two reacting chemical
species.

A

double displacement rxn

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12
Q

common types of double displacement

A

neutralization
and precipitation reactions.

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13
Q

when a
substance reacts with O2 gas to produce
light and heat.

A

conbustion

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14
Q

Represents the main energy level
occupied by electrons.

A

principle quantum number

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15
Q

Is a positive integer, greater than or
equal to 1.

A

principle quantum number (n)

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16
Q

maximum number of electrons
that an electron shell can hold is
given by the formula:

A

2n squared

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17
Q

Describes the shape of the subshells
or the orbital shape within each
principal energy level

A

Azimuthal Quantum Number (l)

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18
Q

possible values of the azimuthal
quantum number

A

all integers between 0 and n-1

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19
Q

l=0

A

s subshell

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20
Q

l=1

A

p subshell

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21
Q

l=2

A

d subshell

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22
Q

l=3

A

f subshell

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23
Q

how many e can s sub shell hold

A

2

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24
Q

how many e can p sub shell hold

A

6

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25
Q

how many e can d sub shell hold

A

10

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26
Q

how many e can f sub shell hold

A

14

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27
Q

which orbital is spherical

A

s

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28
Q

which orbital is shaped like dumbbells

A

p

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29
Q

Describes the orientation of
orbitals in space.

A

Magnetic Quantum Number (ml)

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30
Q

The magnetic quantum number
ranges between

A

the negative and
positive magnitude of the azimuthal
quantum number.

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31
Q

Describes the angular momentum of
an electron.

A

Spin Quantum Number (ms)

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32
Q

Spin Quantum Number (ms) denoted as either

A

+1/2 or -1/2

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33
Q

states that no two electrons in an
atom can have the exact same set of four
quantum numbers.

A

Pauli’s Exclusion
Principle

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34
Q

s sub shell has how many orbitals

A

1

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35
Q

p sub shell has how many orbitals

A

3

36
Q

d sub shell has how many orbitals

A

5

37
Q

f subshell has how many orbitals

A

7ho

38
Q

how many e per orbital

A

2

39
Q

4s subshell gets
filled BEFORE

A

3d bc its lower in energy

40
Q

When two
species have the same electron configuration, it
means that they have the same arrangement of
electrons. They are known as

A

isoelectronic species

41
Q

formed between two atoms
with significantly different electronegativities. (metals and nonmetals)

A

ionic bond

42
Q

involve the complete transfer of
electrons from the less electronegative atom to
the more electronegative atom.

A

ionic bond

43
Q

crystalline structures are found in what kind of bond

A

ionic

44
Q

very high
melting and boiling points are characteristics of what bond

A

ionic

45
Q

soluble in water,
where they dissociate into cations and
anions. translate to what bodn

A

ionic

46
Q

conduct electricity
when dissolved in aqueous solutions or
when they are melted.

A

ionic compound

47
Q

bonds formed between
two atoms that have similar electronegativities. (nonmetal-nonmetal)

A

covalent bond

48
Q

do covalent bonds share e

A

yes

49
Q

which e do covalent bonds share

A

valence

50
Q

have lower
melting and boiling points. what bond

A

covalent

51
Q

are covalent bonds soluble or insoluable

A

insoluable

52
Q

do covalent bonds conduct electricity

A

no

53
Q

describes the distance between
the nuclei of each atom involved in the bond.

A

bond length

54
Q

describes the energy needed to
break a covalent bond.

A

bond energy

55
Q

have their
atoms covalently bonded into a network.
These atoms are held together very tightly,
even tighter than most other covalent
compounds!

A

covalent network solids

56
Q

utilize a
type of covalent bonding whereby both
electrons involved in the bond come from the
same atom.

A

Coordinate covalent compounds

57
Q

utilize a
type of covalent bonding whereby both
electrons involved in the bond come from the
same atom.

A

Coordinate covalent compounds

58
Q

occurs between metal atoms.

A

metallic nond

59
Q

A metallic bond arises
from the

A

electrostatic force between the
delocalized electrons and positively charged
metal ions.

60
Q

excellent conductors
of electricity.. what bond?

A

metallic bond

61
Q

ductile… what bond?

A

metallic

62
Q

malleable… what bond

A

metallic

63
Q

lustrous, or
shiny…. what bond

A

metallic

64
Q

The forces that form covalent or ionic bonds
are termed as

A

intramolecular forces

65
Q

the forces found between molecules.

A

intermolecular forces

66
Q

the weakest intermolecular interactions.

A

London Dispersion / Van der Waals forces

67
Q

occurs when the electron density between
two atoms becomes unevenly distributed for a
brief time resulting in an instantaneous dipole.

A

London Dispersion / Van der Waals forces

68
Q

All compounds
experience the

A

LDF

69
Q

London Dispersion forces get larger as the size
of the molecule

A

increass

70
Q

occurs when the
partially positive side of a molecule attracts the
partially negative side of another molecule.

A

dipole dipole forces

71
Q

interaction is only found in polar solid and
liquid compounds

A

dipole dipole

72
Q

strong dipole-dipole
interactions that occur when hydrogen is
attached to highly electronegative nitrogen,
oxygen, or fluorine atoms.

A

hydrogen bonds

73
Q

what elements are involved in hydrogen bonds

A

nitrogen, oxygen, flourine

74
Q

stronger
than other dipole-dipole interactions.

A

hydrogen bonding force

75
Q

describe the attraction
between an ion and polar molecule.

A

ion dipole interactions

76
Q

increasing the strength of intermolecular forces
implies that these molecules are held…

A

more tightly together

77
Q

does Increasing Intermolecular Forces increase or decrease vapor pressure

A

decrease

78
Q

does Increasing Intermolecular Forces increase or decrease melting and boiling pts

A

increase

79
Q

does Increasing Intermolecular Forces inc or dec viscocity

A

increasedoes

80
Q

does Increasing Intermolecular Forces inc or dec surface tension

A

increase

81
Q

illustrates that
bonding between two atoms occurs due to the
overlap of their atomic orbitals.

A

molecular orbital theory

82
Q

Species that have unpaired electrons and are
attracted to a magnetic field are known as

A

paramagnetic

83
Q

single bond has a bond order of what

A

1

84
Q

triple bond has bond order of what

A

3

85
Q

when a central atom is
surrounded by 3 electron domains, the
atoms arrange themselves to be 120° apart
from each other.

A

trigonal planar

86
Q

when a central atom is
surrounded by 5 electron domains, the
atoms arrange themselves to form this
3-dimensional shape

A

trig bipyrimidal

87
Q

when an atom forms four bonds,
it assumes a…

A

tetrahedral geometry

chem (12 decks)

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