quiz 7

Question 1

valence electrons

Answer 1

electrons on the outermost principle energy level. find val e- for non-transition metal elements by ascending from 1 val e- for group 1 , skipping the transition metals to assign group 13 3 val e-

Question 2

lewis structures for ionic compounds

Answer 2

• for cation, draw lewis structure w 0 electrons inside bracket (ex [na]) and add charge, write shorthand underneath (ex: [he] for na since na+ lost one electron to become he)
• do same for anion except its 8 electrons instead of 0
• dont draw bonds since the bond is ionic and thus involves gain/loss in electrons

Question 3

lewis structure for covalent

Answer 3

• determine amount of val e- for each atom and total val e-
• atom w most bonds goes in center
• at least 1 bond between each atom, up to 3 bonds

Question 4

trick for drawing lewis structure of covalent compounds with non-metals

Answer 4

• # of bonds is 8-[# of val e-]
• # of lone pairs is 4-[# of bonds]
• ex: N has 5 val e- and therefor 8-5=3 bonds, and then 4-3=1 lone pair

Question 5

lewis structure of polyatomic ions

Answer 5

contains covalent bonds within the polyatomic ion with +/- outside of brackets

Question 6

problem solving for ch 10

Answer 6

molecular formula -> lewis structure -> vsepr -> net dipole

Question 7

electron groups of central atom

Answer 7

• leads you to the electron geometry

- # of atoms bonded to central atom + # of lone pairs bonded to central atom

Question 8

electron geometry with 2 electron groups

Answer 8

• electron geometry is linear

- 180 degree (if there are lone pairs, >180)

Question 9

electron geometry with 3 electron groups

Answer 9

• electron geometry is trigonal

- 120 degree (if there are lone pairs, >120)

Question 10

electron geometry with 4 electron groups

Answer 10

• electron geometry is tetrahedral

- 109.5 degree (if there are lone pairs, >109.5)

Question 11

molecular geometry vs electron geometry

Answer 11

• electron geometry depends on electron groups

- molecular geometry makes lone pairs invisible

Question 12

molecular geometry with 2 electron groups

Answer 12

linear

Question 13

molecular geometry with 3 electron groups

Answer 13

• trigonal planar if theres 0 lone pairs

- bent if theres 1 lone pair

Question 14

molecular geometry with 4 electron groups

Answer 14

• tetrahedral if theres 0 lone pairs
• trigonal pyramidal if theres 1 lone pair
• bent if theres 2 lone pairs

Question 15

electronegativity

Answer 15

measure of how much an atom “wants” an electron

increasing as you go up and to the right where F is the most electronegative

Question 16

∆EN

Answer 16

• is EN of atom 1 - EN of atom 2
• ∆EN between 0 - 0.4, then its non polar covalent
• ∆EN between 0.4 - 2, its polar covalent
• ∆EN over 2, its ionic

Question 17

dipole arrow

Answer 17

• points toward more EN atom

- + end aligns with lowercase delta +

Question 18

net dipole

Answer 18

• must be drawn on correct vsepr geometry

- summarizes overall dipole

Question 19

pressure

Answer 19

• force/area

- for gas equations, use atm

Question 20

air pressure goes from

Answer 20

higher to lower pressure

Question 21

less air above you, the less/more air pressure

Answer 21

LESS air pressure

Question 22

boyle’s law

Answer 22

• studies v (volume) and p (pressure), where n (mols) and T (temp) are constant
• p*v=constant since they are inversely proportional

Question 23

charles’ law

Answer 23

• studies V (volume) and T (temp)

- V/T=constant since they are directly proportional

Question 24

avogadro’s law

Answer 24

-studies V (volume) and n (mols)

V/n= constant since they are directly proportional

Question 25

STP

Answer 25

standard temp and pressure, 0 C and 1 atm

Question 26

daltons law of partial pressures

Answer 26

partial pressure of one component = total pressure * fraction of component present

Question 27

resonance hybrid

Answer 27

• occurs when there are multiple acceptable structures
• draw the least common amount of lone pairs and least common amount of bonds, then draw an extra dashed bond
• usually occurs when the compound is charged