Chem 101 Ch.6

Front 1

Metals ___ valence electrons

Back 1

Lose

Front 2

Nonmetals ___ valence electrons

Back 2

Gain

Front 3

Ionic bonds

Back 3

One element stealing electrons from another to try and complete itself

-Transition metals are only ionic

Front 4

Covalent bonds

Back 4

Combining of elements to complete each other's octets

Front 5

Ionic compounds

Back 5

Consists of negative and positive ions, very strong attraction, have high melting and boiling points, are solid at room temperature

Front 6

Transition metals

Back 6

Form positive ions, can only be ionic compounds

Zn^+2, Ag^+1, Cd^+2

Front 7

OH^-1

Back 7

Hydroxide

Front 8

NH4^+1

Back 8

Ammonium

Front 9

NO3^-1

Back 9

Nitrate

Front 10

NO2^-1

Back 10

Nitrite

Front 11

ClO4^-1

Back 11

Perchlorate

Front 12

ClO3^-1

Back 12

Chlorate

Front 13

ClO2^-1

Back 13

Chlorite

Front 14

ClO^-1

Back 14

Hypochlorite

Front 15

CO3^-2

Back 15

Carbonate

Front 16

HCO3^-1

Back 16

Hydrogen carbonate (bicarbonate)

Front 17

CN^-1

Back 17

Cyanide

Front 18

C2H3O2^-1

Back 18

Acetate

Front 19

SO4^-2

Back 19

Sulfate

Front 20

HSO4^-1

Back 20

Hydrogen sulfate (bisulfate)

Front 21

SO3^-2

Back 21

Sulfite

Front 22

HSO3^-1

Back 22

Hydrogen sulfite (bisulfite)

Front 23

PO4^-3

Back 23

Phosphate

Front 24

HPO4^-2

Back 24

Hydrogen phosphate

Front 25

H2PO4^-1

Back 25

Dihydrogen phosphate

Front 26

PO4^-3

Back 26

Phosphate

Front 27

Covalent bonds

Back 27

Form when atoms share electrons to complete octets

Between two nonmetal atoms from Groups 4A, 5A, 6A, 7A

Hydrogen on the outside always, can only have 2 electrons around them, normal elements can have 8

Front 28

Diatomic elements (make up the 7 shape + Hydrogen)

Back 28

H2, N2, O2, F2, Cl2, Br2, I2

Front 29

Lewis Dot structure

Back 29

Hydrogen on the outside always, can only have 2 electrons around them, normal elements want 8

Element that goes in the middle is the one with the least electronegativity (farthest from the top right)

When connecting between two elements, can only have single, double, or triple lines

Front 30

Prefix 1

Back 30

Mono

Front 31

Prefix 2

Back 31

Di

Front 32

Prefix 3

Back 32

Tri

Front 33

Prefix 4

Back 33

Tetra

Front 34

Prefix 5

Back 34

Penta

Front 35

Prefix 6

Back 35

Hexa

Front 36

Prefix 7

Back 36

Hepta

Front 37

Prefix 8

Back 37

Octa

Front 38

Prefix 9

Back 38

Nona

Front 39

Prefix 10

Back 39

Deca

Front 40

Nonpolar covalent bonds

Back 40

Almost no electronegativity difference (0-.4)

Occurs between nonmetals

Front 41

Polar covalent bonds

Back 41

Moderate electronegativity difference (.5-1.7)

Occurs between nonmetal atoms

Front 42

Ionic bonds

Back 42

Large electronegativity difference (1.8+)

Occurs between metal and nonmetal ions

Front 43

Beryllium (Be)

Back 43

Can be Electrodeficient, it can have four if needed

Front 44

Two bonded atoms (BeCl2)

Back 44

Linear shape, 180°

Front 45

Three bonded atoms (BF3)

Back 45

Trigonal planar, 120° w/ 3 atoms attached to B

Front 46

Two bonded atoms and one lone pair (SO2)

Back 46

Bent, 120 degrees w/ 2 atoms bonded to S

Front 47

4 bonded atoms (CH4)

Back 47

Tetrahedral shape, 109° arrangement

Front 48

Three bonded atoms and one lone pair (NH3)

Back 48

Tetrahedral arrangement, the three bonded atoms form a pyramidal 109° shape

Front 49

Two bonded atoms and two lone pairs (H2O)

Back 49

Tetrahedral arrangement, the two bonded atoms form a bent 109° shape

Front 50

Dipole-dipole attractions

Back 50

In covalent compounds, polar molecules with no hydrogen bonds

The bonds are different nonmetals

Front 51

Hydrogen bonds (special Dipole-dipole attractions)

Back 51

Hydrogen connected to certain elements like (O-H, F-H, N-H)

Front 52

Dispersion forces

Back 52

Weak attraction between nonpolar molecules (F-F), caused by temporary dipoles that develop when electrons are not distributed equally

Front 53

Molecules delta's

Back 53

The lone pair determines where the plus or minus Delta is

Front 54

Comparison of bonding and attractive forces

Back 54

Strongest ---> Weakest

Ionic bonds (Na-Cl), hydrogen bonds (H-F, H-N, H-O), dipole-dipole attractions (Br-Cl), dispersion forces (F-F)

Front 55

Melting point and attractive forces

Back 55

Ionic compounds require large amounts of energy to break apart ionic bonds, thus they have high melting points

Hydrogen bonds are the strongest type of dipole-dipole attractions, they require more energy to break than do other dipole attractions

Dispersion forces are weak interactions, and very little energy is needed to change their state