unit 5 test

Question 1

valence electrons

Answer 1

s and p electrons in outer energy level (only valence electrons participate in chemical reactions)

Question 2

core electrons

Answer 2

all the rest electrons in lower energy level (do not participate in chemical reactions)

Question 3

group 1

Answer 3

1 valence electron
1+ charge

Question 4

group 2-12

Answer 4

2 valence electron
2+ charge

Question 5

group 13

Answer 5

3 valence electron
3+ charge

Question 6

group 14

Answer 6

4 valence electron
3- charge
4 bonds

Question 7

group 15

Answer 7

5 valence electrons
3- charge
3 bonds

Question 8

group 16

Answer 8

6 valence electrons
2- charge
2 bonds

Question 9

group 17

Answer 9

7 valence electrons
1- charge
1 bond

Question 10

group 18

Answer 10

8 valence electrons

Question 11

ions

Answer 11

negative and positive atoms transferring valence electrons

Question 12

ionic bonds

Answer 12

metals and nonmetals

Question 13

1 to 4 valence electrons

Answer 13

lose electrons to become cations

Question 14

5 to 7 valence electrons

Answer 14

gain electrons to become anions

Question 15

formula unit

Answer 15

lowest ratio of elements that represent the resulting ionic compound (like empirical)

Question 16

covalent bonds

Answer 16

share electrons (nonmetals to nonmetals)

Question 17

molecular formula

Answer 17

the exact number of atoms in a molecule (not simplified)

Question 18

structural formula

Answer 18

shows all the details how atoms are connected (most accurate or detailed)

Question 19

diatomic elements

Answer 19

Br, I, N, Cl, H, O, F

Question 20

polar

Answer 20

unevenly shared (0.4 to 2.0)
attracts electrons to spend more time around the most negative

Question 21

nonpolar

Answer 21

evenly shared (0 to 0.4) identical nonmetals are always nonpolar

Question 22

intermolecular forces (IMF)

Answer 22

weaker attractive forces between molecules

stick due to polarity
hydrogen is most significant (H to N, H to O, H to F)

Question 23

ionic compound properties

Answer 23

high melting points
hard and brittle solid form (crystalline)
conducts electricity

Question 24

covalent compound properties

Answer 24

low melting point
soft or brittle solid form (amorphous)
poor conductivity
does not dissociate in water

Question 25

metallic compound properties

Answer 25

high melting point hard yet malleable solid form conducts electricity

Question 26

VSEPR theory

Answer 26

Valence Shell Electron Pair Repulsion electron pairs stay away from each other as much as possible

Question 27

4 electron groups

Answer 27

109.5 tetrahedral (nonpolar) pyramidal (polar) bent (polar)

Question 28

3 electron groups

Answer 28

120 trigonal planar (nonpolar) bent (polar)

Question 29

2 electron groups

Answer 29

180 linear (nonpolar)

Question 30

transition metals

Answer 30

can vary charges - charges shown as roman numerals exceptions are Ag(1+), Zn(2+), Cd(2+)

Question 31

monoatomic anions always end with

Answer 31

-ide

Question 32

polyatomic anions can end with

Answer 32

-ide, -ate, -ite

Question 33

ionic compound formulas are found using

Answer 33

the criss cross rule find the charge, mulitply by the number of atoms, swap

Question 34

prefixes for elements (1-10)

Answer 34

mono di tri tetra penta hexa hepta octa nona deca

Question 35

which two elements have different bond needs?

Answer 35

boron (6) hydrogen (2)

Question 36

when are prefixes used?

Answer 36

when no metals are present

Question 37

intermolecular forces: dispersion forces

Answer 37

present in every molecule (non/polar) attraction with two random dipoles asymmetrical electron distribution weakest relative strength

Question 38

intermolecular forces: dipole dipole forces

Answer 38

present in polar molecules attraction with two permanent dipoles medium relative strength

Question 39

intermolecular forces: hydrogen bonding

Answer 39

present whenever H is bonded with O, N, or F extremely polar bonds (very strong dipole force) not chemical bonding

Question 40

hybridization

Answer 40

the process in which atomic orbitals are mixed to form new identical orbitals for bonding

Question 41

single bond in hybridization

Answer 41

sigma bond (special o)

Question 42

double or triple bond in hybridization

Answer 42

pi bond (pi sign) stronger than single bond

Question 43

4 valence electrons in hybrid

Answer 43

sp3 (no p orbitals to make a pi bond)

Question 44

3 valence electrons in hybrid

Answer 44

sp2 (1 p orbital to make a pi bond)

Question 45

2 valence electrons in hybrid

Answer 45

sp (2 p orbitals to make 2 double or triple bond)

Question 46

isomer

Answer 46

molecule with the same formula but different arrangement of atoms in molecule

Question 47

molecule

Answer 47

two nonmetals (a covalent bond)