Atomic and Molecular Structure

Question 1

Dalton’s atomic theory explains that all matter is made up of -__ which are ___. And that all atoms of a given element are identical in __ and ___

Answer 1

atoms, indivisible, mass, property

Question 2

___ electrons are all electrons except the valence electrons, and the number of electrons in each energy level is equal to ____

Answer 2

core, 2n^2

Question 3

atoms of the same element that have the same number of protons but different number of neutrons

Answer 3

isotopes

Question 4

involves changes to the physical properties of a substance; no new products are formed and no new chemical bonds are formed or destroyed

Answer 4

physical reactions

Question 5

When bonds are formed or broken and new substances are made

Answer 5

chemical reaction

Question 6

When two different compounds come together to form a single compound; usually release energy

Answer 6

synthesis

Question 7

When a compound breaks down into two or more products; require energy

Answer 7

decomposition

Question 8

When one element replaces another in a compound

Answer 8

single displacement

Question 9

When two elements replace one another in a compound

Answer 9

double displacement

Question 10

When a substance reacts with O2 to form light and heat

Answer 10

combustion

Question 11

Bohr believed that electrons move in __ __ around the nucleus, but this has since been disproven

Answer 11

fixed orbitals

Question 12

states that it is impossible to know both the exact location and momentum of an electron at the same time

Answer 12

heisenberg’s uncertainty principle

Question 13

the space that is the most probable locations for electrons

Answer 13

electron cloud

Question 14

The __ ___ ___ describes the energy level of the electron, and it must be ____. The maximum number of electrons each level can hold is given by ____. The ___ number on the periodic table represents the energy level of the valence electrons

Answer 14

principle quantum number, N>=1, 2n^2, row

Question 15

the __ __ __ describes the orbital shape, and can be between __ and ___.

Answer 15

azimuthal quantum number, 0, n-1

Question 16

When l = 0, the subshell is ___, which is ___ shaped, when l=1 the subshell is ___ which is ____ shaped, when l=2 the subshell is ____ which is ___ shaped and when l=3, the subshell is ___

Answer 16

s, spherical p, dumbell, d, clover, f

Question 17

The magnetic quantum number describes the __ ___ in space, and takes the value of __ and ___

Answer 17

orbital orientation, -l, +l

Question 18

The __ ___ __ describes the angular momentum of the electron and can be either __ or ___

Answer 18

spin quantum number, -1/2, +1/2

Question 19

Says that no two electrons within an atom can have the exact same quantum numbers

Answer 19

pauli’s exclusion principle

Question 20

The s orbital has __ electrons, the p orbital has ___ electrons, the d orbital has ___ electrons, and the f orbital has ___ electrons

Answer 20

2, 6, 10, 14

Question 21

describes the number of electrons in each energy level and the order in which subshells are filled

Answer 21

electron configuration

Question 22

In electron configuration notation, the first number describes the __ __ __, and the letter describes its ___, the superscript describes the number of ___ in it

Answer 22

principle energy level, subshell, electrons

Question 23

the alkali and alkaline earth metals are the ___ block, the nonmetals are the ___, the transition metals are the __, and the lanthinide and actinides are the ___ block

Answer 23

s, p, d, f

Question 24

says that subshells tend to get filled from lower energy to higher energy

Answer 24

aufbau principle

Question 25

Says that all orbitals of a subshell are first singly occupied before they are doubly occupied

Answer 25

hund's rule

Question 26

Exceptions to the electron configurations occur when elements like to have ___ or ___ ___ subshells. This includes elements like __, __ and ___, ___, ___

Answer 26

full, half full, Cr, Mo, Au, Ag, Cu

Question 27

Valence electrons are always removed first from the __ ____ subshell

Answer 27

highest energy

Question 28

When two species that have the same electronic configurations

Answer 28

isoelectronic species

Question 29

Ionic compounds are ___ __ that have high melting and __ ___, are soluble in ___, and __ __ in aqueous and __ forms

Answer 29

crystalline solids, boiling points, water, conduct electricity, molten

Question 30

Covalent compounds have weaker bonds than ionic, thus have lower _- and ___ points, are ___ or ___ at room temperature, are __ in water, and do not conduct ___

Answer 30

melting, boiling, liquid, gas, insoluble, electricity

Question 31

distance between the each atom in a covalent bond; decreases as the number of electron pairs shared increases

Answer 31

bond length

Question 32

The energy needed to break the covalent bond; increases as the electron pairs shared increases

Answer 32

bond energy

Question 33

distribution of charges

Answer 33

polarity

Question 34

When atoms of a chemical compound are covalently bonded in a network

Answer 34

covalent network solid

Question 35

Examples of covalent network solids are __ and ___

Answer 35

diamond, quartz

Question 36

When in a covalent bond, both electrons come from the same atom

Answer 36

coordinate covalent

Question 37

electrostatic attractive force between delocalized electrons and positively charged metal ions

Answer 37

metallic bond

Question 38

Metallic compounds like __ and __ fused together, conduct ___, are ___, ___, and ___

Answer 38

gold, silver, electricity, ductile, malleable, lustrous

Question 39

dipole dipole interactions does not occur in ____ because the molecules are too far apart.

Answer 39

gasses

Question 40

Ion dipole interactions are the attraction between the ____ and ___ molecules, and are stronger than dipole dipole interactions,

Answer 40

ions, polar

Question 41

Increasing the intermolecular forces increases the __ and __ points, the ___, the __ __, and decreases the __ ___

Answer 41

melting, boiling, viscosity, surface tension, vapor pressure

Question 42

The __ ___ rule applies to hydrogen, helium, ____, ____, ___ and -__

Answer 42

reduced octet, lithium beryllium, boron, aluminum

Question 43

___ ___ is when elements have more than 8 outer electrons and apply to elements within the __ row or more that have a __ subshell

Answer 43

exceeding octet, 3rd, d

Question 44

the central atom is the one that can make the most __, and is usually the __ ___ atom. It is also usually ___

Answer 44

bonds, least electronegative, carbon

Question 45

___ and ___ will never be the central atom, and will only form one bond.

Answer 45

hydrogen, halogens

Question 46

the formula for formal charge

Answer 46

number of valence electrons - non bonding electrons - number of bonds

Question 47

Bonding occurs when orbitals with electrons ___. When this happens, the atomic orbitals are ____ into shapes that resemble the atomic orbitals. This forms a __ ___. The number of orbitals must be ___. Hybrid orbitals have better __ and form ___ bonds

Answer 47

overlap, hybridized, covalent bond, conserved, overlap, stronger

Question 48

sigma bonds allow for __ __ about its axis, whereas ___ bonds do no

Answer 48

free rotation, pi

Question 49

All single bonds are ___ bonds. A double bond has ___ pi bond and a triple bond has ___ pi bonds

Answer 49

sigma, 1, 2

Question 50

the number of lone pairs or bond locations around an atom

Answer 50

number of lone pairs or bond locations around an atom

Question 51

Double and triple bonds only count as ___ electron domain

Answer 51

1

Question 52

The bond order is equal to

Answer 52

number of bonding orbital electron - number of antibonding orbital electron / 2

Question 53

bond order is equal to the number of ___

Answer 53

bonds

Question 54

an atom that has one or more unpaired electrons and thus is attracted to a magnetic field

Answer 54

paramagnetic

Question 55

when an element has no unpaired electrons and thus repels a magnetic field

Answer 55

diamagnetic

Question 56

As the bond order increases, the bond strength ____. An increase in ___ __ produces a decrease in bond strength. The greater the ____, the greater the bond strength. The presence of less ___ ___ indicates a greater bond strength

Answer 56

increase, atomic radii, polarity, lone pairs

Question 57

VSPER theory determines the __ __ of ___ molecules. Electron pairs ___ each other and will arrange themselves as far apart as possible

Answer 57

geometric arrangement, covalent, repel,

Question 58

has 2 electron domains and 180° separation

Answer 58

linear

Question 59

has 3 electron domains and 120° separation

Answer 59

trigonal planar

Question 60

has 4 electron domains and 109.5° separation

Answer 60

tetrahedral

Question 61

Has 5 electron domains with 90°, 180°, and 120° separations

Answer 61

trigonal bipyramidal

Question 62

Has 6 electron domains with 90° separation

Answer 62

octahedral

Question 63

a bent shape that occurs with ___ bonds and __ lone pair has a bond angle of ___ 120°

Answer 63

2, 1, <

Question 64

a trigonal pyramidal shape that occurs due to ___ bonds and __ lone pair has a bond angle of ___

Answer 64

3, 1, 107.5°

Question 65

The bent shape created by __ bonds and ___ lone pairs has a bond angle of ___

Answer 65

2, 2, 104.5°

Question 66

a ____ shape is formed with 4 bonds and 1 lone pair, with angles that are greater than __ and ___

Answer 66

seesaw, 90, 120

Question 67

A ____ shape results from 3 bonds and 2 lone pairs, and has a bond angle of ___90

Answer 67

t, <

Question 68

a ___shape can result from a molecule of 2 bonds and 3 lone pairs, and has a bond angle of ___

Answer 68

linear, 180°

Question 69

a ___ __ shape results from a molecule with 5 bonds and 1 lone pair and its bond angle is ____ 90

Answer 69

square pyramidal, <

Question 70

A __ __ shape results from a molecule with 4 bonds and 2 lone pairs and has a bond angle of ____

Answer 70

square planar, 90°