Exam 3: Definitions

Question 1

Ionic compounds

Answer 1

Metal + nonmetal

dissolves in water

Question 2

molecular compound

Answer 2

nonmetals

Question 3

Electronegativity

Answer 3

    | ----> 

right and up. Top right

Question 4

increasing boiling point

Answer 4

more bonds = more energy to melt

H bonds are weak but H-H bonds are weaker

double/tripple bonds = more energy to break

bigger size = more energy to break

more heat = more breaking of bonds

Question 5

The numerical value of an element’s electronegativity represents….

Answer 5

the ability of an atom in a bond to draw shared electrons to itself

Question 6

Radical

Answer 6

1 atom has an odd number of electrons (after bonding everything after)

Question 7

dipole- dipole

Answer 7

Next strongest

attractive forces between the positive end of one polar molecule and the negative end of another polar molecule

Question 8

Hydrogen bonding

Answer 8

Can attract other molecules that are SIMILAR

ONLY occurs between molecules with Hydrogen bonded to high electronegative elements like N, O, F

Question 9

london dispersion forces

Answer 9

Weakest bond compared to dipole-dipole and hydrogen bonding

everything is attracted to the dispersion force (bigger molecule = bigger dispersion force)

weak = gas
strong = solids

Question 10

Electron domains

Answer 10

lone pairs,
single, double, tripple bonds

Question 11

valance bond theory describes how a covalent bond is formed by….

Answer 11

the overlap of two orbitals, with each orbital containing one electron

Question 12

polar

Answer 12

dipole

London dispersion and dipole-dipole

lower it is on PT = lower polarity

Polar/ Polar covalent (e shared UNequally) : .5-2

BOTH need to be met or else its non-polar:

1)central atom has no lone pairs

2)all atoms around the central atom are the same

Question 13

non-polar

Answer 13

no dipole

London dispersion

ONLY ONE needs to be met:

1) the central atom has no lone pairs

2) all atoms around the central atom are the same

Non-polar / covalent (e shared equally): less than .5

has symmetry

Question 14

dipole

Answer 14

based on electronegativity
difference in electrons

lightly charged on one side than other

Question 15

When a covalent bond forms between two atom, the potential energy of the system ______. To break a bond, energy must be ______.

Answer 15

Decrease
added

Question 16

Octet rule states

Answer 16

atom gains, lose, or share electrons so that they end up with a full outer shell

Question 17

valence bond theory describes how a covalent bond is formed by…

Answer 17

the overlap of two orbitals, with each orbital containing one electron

Question 18

lone pairs

Answer 18

2 electrons (pair)

Question 19

Polyatomic ions

Answer 19

Charged ions

Question 20

Resonance

Answer 20

when two or more L.S with atoms in the same position are averaged to gove the true structure

Question 21

The ability of a bonded atom to draw shared electrons to itself is called…

Answer 21

electronegativity

Question 22

Boiling point question: atmosphere pressure and room temp, bromine is a liquid, and iodine is a solid. we can conclude that bromine….

Answer 22

has weaker intermolecular forces that iodine

(bromine is weaker cuz bonds broke and turned into liquid)

Question 23

Attractions

Answer 23

Like attractions: repel
Opp attractions: attract

Question 24

When a covalent bond forms between two atoms, the potential energy of the system ______. to break a bond, energy must be _____.

Answer 24

decreases
added

Question 25

Periodic table movements

Answer 25

+ means move left

• means move right

Question 27

Lewis Structure movements

Answer 27

Add electrons for NEG charges

Sub electrons for POS charges

Question 28

Lewis structure drawing additions

Answer 28

+ for Lewis structure if L.S needs to LOSE electrons

– for Lewis structure if L.S needs to GAIN electrons

Question 29

ion-induced dipole

Answer 29

attraction between ionic and nonpolar

Question 30

Ion-dipole

Answer 30

Atrraction between ionic and polar

Question 31

Covalent bonds

Answer 31

SHARED bonds, not transfer

Question 32

intermolecular forces

Answer 32

keeps everything tohether

Question 33

polymers

Answer 33

chain of repeating molecules

Question 34

Distinguish if bonds are polar, non-polar, or ionic

Answer 34

Polar/ Polar covalent (e shared equally) : .5-2
Non-polar / covalent (e shared UNewually): less than .5
Ionic (transferred bonds) : 2.0 or more

Question 35

Compounds with H-F, H-N

Answer 35

London dispersion, dipole-dipole, hydrogen bond