E.4_ch.8.9_

Question 1

What is a ionic bond?

Answer 1

electron transfer between metals and nonmetals

Question 2

What is a covalent bond?

Answer 2

electron sharing between nonmetals

Question 3

What is a metallic bond?

Answer 3

electron pooling between metals

Question 4

What do Lewis Symbols help predict?
What does the symbol represent?
What does the dots represent?

Answer 4

bonding

nucleus and core electrons

valence electrons

Question 5

What is the number of valence electrons on the periodic table?

Answer 5

the A group number

Question 6

What do lewis symbols number of dots tell us?

Answer 6

for main group metals, they equal the number of electrons the atom loses to form a cation

for nonmetals, they equal the number of electrons the atom gains to form a anion

Question 7

Who created the octet rule?

Answer 7

Gilbert Lewis (1916)

Question 8

What is the octet rule?

Answer 8

bonded atoms either gain, lose, or share electrons to attain a filled outer layer of 8 e-

atoms like to achieve noble gas configurations

Question 9

What does the octet rule apply to?

Answer 9

almost all compounds made of the period 2 elements and some others

Question 10

Why do ionic bonds cause attraction between 2 atoms?

Answer 10

transfer of electrons = opposing charges

Question 11

What is ionization energy?

Answer 11

The energy absorbed by 1 mole of an atom when it loses 1 mole of electrons

Question 12

What is electron affinity?

Answer 12

The energy released by 1 mole of an atom when it gains 1 mole of electrons

Question 13

What is a lattice?

Answer 13

The structure of a crystalline solid formed from the attraction of multiple ions

Question 14

What is lattice energy?

Answer 14

The energy to separate 1 mole of a solid to form 1 mole of gaseous ions

Question 15

What kind of energy to atoms want?

Answer 15

Energy kept to a minimum

Question 16

What happens to the overall energy when ionic bonds form?

Answer 16

Energy is released

Overall energy lowers

Question 17

What are the physical behavior of an ionic solid?

Answer 17

Ionic solid is hard, rigid, and brittle

Question 18

What are the electrical conductivity of an ionic solid?

Answer 18

Ionic solid does not conduct electricity, but it does once melted or dissolved

Question 19

What are the thermal conductivity of an ionic solid?

Answer 19

In the normal state, there is no such thing as an individual ionic molecules, just interconnected solids or arrays

Question 20

What must we understand to understand why and how covalent bonds are formed?

Answer 20

Electro negativity

Question 21

What is electronegativity not the same as ?

Answer 21

Electron affinity

Question 22

Who discovered electronegativity?

Answer 22

Linus Pauling (1932)

Question 23

What is electronegativity?

Answer 23

The relative ability of a bonded atom to attract shared electrons

Question 24

What are electronegativity values relative to?

Answer 24

The greatest value of 4.0 which is fluorine

Question 25

How is electronegativity related to size?

Answer 25

EN is inversely related to size Smaller the atom ... the closer the shared pair can get to the nucleus

Question 26

Do electrons share equally when a covalent bond is formed?

Answer 26

No

Question 27

What is a unequal sharing of electrons?

Answer 27

Polar covalent bond

Question 28

What is an equal sharing of electrons?

Answer 28

No polar covalent bond

Question 29

What is used to determine bond polarity ?

Answer 29

Electronegativity

Question 30

What sharing does two atoms of the same element form when bonded?

Answer 30

Equal sharing of electron | Non polar covalent bond

Question 31

What sharing does two atoms of different elements form when bonded?

Answer 31

Unequal sharing of electrons | Polar covalent bond

Question 32

What charge does the most electronegative element get? The least electronegative?

Answer 32

Most EN = partial negative charge | Least EN = partial positive charge

Question 33

What helps is determine bond polarity?

Answer 33

The difference in electronegativity between two bonded species

Question 34

Names the name— EN difference — bond type — example ... What’s the biggest difference in EN

Answer 34

Zero — (0-0.4) — polar covalent — Cl2 Intermediate — (0.4-2.0) — polar covalent — HF Large — (2.0+) — ionic — NaCl 3.3

Question 35

What is the difference between bond polarity and molecular polarity?

Answer 35

Bond polarity: if bond is polar or not Molecular polarity: if molecule is polar or not

Question 36

What do Lewis structures and Lewis symbols describe?

Answer 36

Lewis symbols : single atom Lewis structures : molecules

Question 37

What is a Lewis structure an outline for?

Answer 37

Bonding and arrangement of atoms in a molecule

Question 38

What is a resonance structure?

Answer 38

The different Lewis model structures that can be made

Question 39

What are equivalent resonance structures and what are no equivalent resonance structures?

Answer 39

Equivalent resonance structures: mirrored No equivalent resonance structures: not the same/mirrored

Question 40

What structure is the real molecule when choosing a where the double bond goes?

Answer 40

Hybrid

Question 41

How is the bonding order calculated?

Answer 41

Bond Order = Bonding pairs / Atom pairs

Question 42

How do we represent ions in a Lewis structure?

Answer 42

Braquets and charge outside top right corner

Question 43

When do we want to limit formal charges on Lewis structures?

Answer 43

When we have non equivalent resonance forms

Question 44

How do you calculate the formal charge?

Answer 44

FC= # valence e - # unshared e - (1/2)(# shared e)

Question 45

What do the FC added together equal?

Answer 45

The charge of the ion molecule

Question 46

What is the best resonance form ?

Answer 46

Limits formal charge Places negative charge on the most EN atom (Places positive charge on lease EN atom)

Question 47

What happens to the d(distance form nucleuses) and lattice energy as the size of ions increase?

Answer 47

d increases | LE decreases

Question 48

What two things can coulombs law predict?

Answer 48

strength of ionic bond | lattice energy

Question 49

What kinds of ions and charges do we want?

Answer 49

small ions large charges = high LE

Question 50

What is the equation for coulombs law?

Answer 50

E ∝ (q1q2)/d ∝ LE

Question 51

Do lewis structures tell us anything about the shape of the molecule?

Answer 51

no

Question 52

What are the five rules of lewis structures?

Answer 52

hydrogen can only form one bond and can never be a central atom no matter what EN halogens generally form 1 bond and are generally surrounding atoms carbon forms 4 bonds nitrogen forms 3 bonds oxygen forms 2 bonds

Question 53

What are the three ways an octet rule can disobey the octet rule ?

Answer 53

electron deficient atom odd electron atom atoms with expanded valence shells

Question 54

What are electron deficient atoms and what are examples?

Answer 54

these atoms often have fewer than 8 electrons around them when they are the central atom Be and B when not central is willing to follow octet rule after bond

Question 55

What are odd electron atoms and what is an example?

Answer 55

electrons don't always come in pairs leaves one electron by itself NO2

Question 56

What is it called when one electron is left by itself on a lewis dot structure?

Answer 56

free radicals

Question 57

What are expanded valence atoms and what is an example?

Answer 57

atoms that expand their valance shells to beyond 8 electrons period 3 or higher sulfur

Question 58

Why can atoms in period 3 or higher bond more than 8 valance electrons?

Answer 58

it has 3d orbitals available to it has 3s and 3p to place electrons

Question 59

Do lewis structures tell us anything about the arrangement of molecules in space?

Answer 59

no

Question 60

What do lewis structures tell us?

Answer 60

used to determine geometry

Question 61

What does molecular shape determine?

Answer 61

functionality

Question 62

What is electron group arrangement?`

Answer 62

the distribution of electrons (shared and unshared) around a central atom

Question 63

What is molecular geometry?

Answer 63

the distribution of the atoms in 3D space

Question 64

What do the following represent for drawing in three dimensions? single lines bold lines dashed lines

Answer 64

bonds in the plane bonds that are angled forward bonds that are angled backward

Question 65

What does VSEPR stand for?

Answer 65

valence-shell electron-pair repulsion

Question 66

What is VSEPR?

Answer 66

the primary theory behind determining molecular geometry, based on 2 principles

Question 67

What are the two principles of the theory of VSEPR?

Answer 67

e pairs repel each other ... occupy space farthest away from each other as possible a bond is sharing electrons ... unpaired electrons are more localized on a single atom

Question 68

How do we use VSEPR?

Answer 68

1. determine the # of e- groups around central atom 2. determine e- group arrangement ( identify optimal bond angles ) 3. consider lone pair repulsion impact on a bond angle 4. determine molecular geometry

Question 69

True or False: double and triple bonds are considered a single e- group?

Answer 69

true

Question 70

In electron group arrangements, the total # of electron groups around a central atom can range from what? Each e- group arrangement will provide us with various possible _______?

Answer 70

2-6 molecular geometries

Question 71

What electron group arrangement is when there are only two electron groups around a central atom? What are the other possible geometries?

Answer 71

linear electrons group arrangement linear is the only one possible