guided notes

Question 1

Atoms form bonds to:

Answer 1

-decrease potential energy
-increase stability

Question 2

Potential energy is decreased as ->

Answer 2

Bond is formed

Question 3

How is a bond formed?

Answer 3

two opp forces of attraction balance at the precise distance where potential energy is at a minimum

Question 4

Forming a chemical bond =

Answer 4

exothermic process (releases energy and stability inc)

Question 5

Breaking a chemical bond=

Answer 5

endothermic process (absorbs energy and Potential energy Inc and stability dec)

Question 6

Compounds have less potential energy than the ->

Answer 6

individual atoms they are formed from (more stable)

Question 7

Atoms gain a stable full valence energy level by ->

Answer 7

bonding with other atoms

Question 8

Octet rule:

Answer 8

bonds form btwn atoms by gaining, losing, or sharing e- in order to have an octet of e-

Question 9

When chemical bonds form, valence e- are: (3)

Answer 9

-transferred from one atom to another (ionic)
-shared btwn atoms (covalent)
-free moving in sea of e- (metallic)

Question 10

The electronegativity difference btwn tow bonded atoms determines _>

Answer 10

type of bond

Question 11

0.0-0.3 =

Answer 11

non polar covalent

Question 12

0.3-1.7=

Answer 12

polar covalent

Question 13

1.7-3.3 =

Answer 13

ionic

Question 14

Two major categories of compounds based on bonding:

Answer 14

Ionic compounds and molecular (covalent ) compounds

Question 15

Ionic compound:

Answer 15

metal bonded with nonmetal or compound containing a polyatomic ion

Question 16

molecular (covalent) compound:

Answer 16

tow or more nonmetals combined

Question 17

Ionic Compound properties:

Answer 17

-high melting point
-high boiling point
-dissolve in water
-conducts electricity in solution and as liquids

Question 18

Covalent (molecular) compound properties:

Answer 18

-lower melting points
-lower boiling points
-do not conduct electricity

Question 19

(ionic bond) metal loses e- to form a

Answer 19

cation (+ ion)

Question 20

(ionic bond) nonmetal gains e- to form a :

Answer 20

anion (- ion)

Question 21

What forms an ionic bond?

Answer 21

an electrostatic attraction

Question 22

covalent bonds:

Answer 22

forec between tow atoms due to a sharing of one or more e-, forming a molecule

Question 23

Metallic bonds:

Answer 23

occurs btwn atoms of metals

Question 24

(metallic bond) Where are the valence e- held?

Answer 24

loosely held in a moble sea of valence e-

Question 25

(metallic Bonding) what does this type of bonding account for?

Answer 25

some unique properties of the unique properties of metals (conduct electricity. luster, and malleability)

Question 26

Lewis Dot Notation:

Answer 26

dots around the element symbol represent the # of valence e-

Question 27

(Lewis structure ions) cation gets a_____ to show loses of e-

Answer 27

bracket

Question 28

(lewis structure ions) Anion gets _______to show gain of e-

Answer 28

full bracket

Question 29

(lewis structure polyatomic ion) polyatomic ions are represented as a ->

Answer 29

complete unit -brackets go around whole structre with charge outside

Question 30

(lewis structures molecular compounds) dashes btwn atoms represent:

Answer 30

covalent bonds

Question 31

VSEPR

Answer 31

valence shell electron pair repulsion theory

Question 32

VSEPR theory predict the:

Answer 32

goemetric shape of the molecule

Question 33

VSEPR Theory:

Answer 33

the repulsion forces of valence-level e- will cause atoms of a molecule to spread out as far apart as possible

Question 34

molecular geometry:

Answer 34

the 3 dimensional arrangement of a molecule's atoms

Question 35

Lone pairs;

Answer 35

pairs of e- not bonded to another atom

Question 36

Linear shape:

Answer 36

2 atoms bonded and 0 lone pairs

Question 37

trigonal planar shape:

Answer 37

3 atoms bonded and 0 lone pairs

Question 38

tetrahedral shape:

Answer 38

4 atoms bonded and 0 lone pairs

Question 39

trigonal pyramidal shape:

Answer 39

3 atoms bonded and 1 lone pair

Question 40

bent

Answer 40

2 atoms bonded and 2 lone pairs

Question 41

Lone pairs repel ->

Answer 41

more strongly that bonded pairs

Question 42

Polar molecules:

Answer 42

dipoles

Question 43

Determine polarity by:

Answer 43

looking for symmetry/ asymetry in lewis structure

Question 44

Direction of the dipole is toward...

Answer 44

most electronegative atom

Question 45

asymetrical=

Answer 45

polar

Question 46

symetrical=

Answer 46

nonpolar

Question 47

intermolecular forces:

Answer 47

forces of attraction that occur between molecules

Question 48

Intramolecular forces:

Answer 48

forces of attraction that occur btwn atoms -covalent bond

Question 49

Intermolecular forces are much _____ than the strong covalent bonds holding molecules together (intra)

Answer 49

weaker

Question 50

Types of intermolecular forces:

Answer 50

-dipole-dipole interactions -London Dispersion forces -Hydrogen bonds

Question 51

Hydrogen bonding:

Answer 51

bond btwn hydrogen and a more electronegative atom (O,N, F)

Question 52

Dipole-Dipole Interactions:

Answer 52

attraction btwn opp charged regions (polar molecules) of neighboring molecules

Question 53

London dispersion forces :

Answer 53

the weaker force cause by motion - momentary force

Question 54

London disepersion force is the only force acting on....

Answer 54

nonpolar molecules and noble gases

Question 55

Hydrogen bond is a special type of....

Answer 55

dipole-dipole force and is the strongest force

Question 56

The strength of the hydrogen bond increases w/...

Answer 56

the degree of electronegativity of the atom bonded to it