chem unit 2 test

electronegativity of H

2.1

electronegativity of Li

1.0

electronegativity of Be

1.5

electronegativity of B

2.0

electronegativity of C

2.5

electronegativity of N

3.0

electronegativity of O

3.5

electronegativity of F

4.0

nitrate

NO3 (1-)

nitrite

NO2 (1-)

carbonate

CO3 (2-)

sulfate

SO4 (2-)

sulfite

SO3 (2-)

phosphate

PO4 (3-)

permanganate

MnO4 (1-)

perchlorate

ClO4 (1-)

chlorate

ClO3 (1-)

chlorite

ClO2 (1-)

hypochlorite

ClO (1-)

ammonium

NH4 (1+)

hydroxide

OH (1-)

cyanide

CN (1-)

electronegativity trend

increases up and to the right

atomic radius

increases down and to the left

lattice energy

higher energy with higher charge and SMALLER atomic radius, lower energy with less charge and BIGGER atomic radius

electronic geometry of 2 RHEDS

linear

hypovalency

fewer valence electrons than usual (B and Be)

number of bonds B forms

3

number of bonds Be forms

2

radical

odd number of total valence electrons

hypervalency

more electrons than usual due to ability to access d orbital (n=3 or higher)

alcohols

OH

aldehyde

CHO

ketone

CO

carboxylic acid

COOH

amines

NH2

amide

CONH2

formal charge formula

total # of valence electrons for an atom - (lines) - (lone pairs)

-1 charge on the more electronegative atom

better structure of atom

not associated with resonance structures

hydrogen or halogens

as bond length increases

bond strength decreases

examples of singular RHEDS

a lone pair, a radical, a single bond, a double bond, a triple bond

3 RHEDS

trigonal planar geometry

tetrahedral geometry

4 RHEDS

trigonal bipyramidal

5 RHEDS

octahedral

6 RHEDS

linear molecular shape (2 rheds)

AB2

trigonal planar molecular shape

AB3

bent molecular shape (3 RHEDS)

AB2U

tetrahedral molecular shape

AB4

trigonal pyramidal molecular shape

AB3U

bent molecular shape (4 RHEDS)

AB2U2

trigonal bipyramidal molecular shape

AB5

seesaw molecular shape

AB4U1

t-shaped molecular shape

AB3U2

linear molecular shape (5 RHEDS)

AB2U3

octahedral molecular shape

AB6

square pyramidal molecular shape

AB5U

square planar molecular shape

AB4U2

180 degree bond angle

linear molecular shape

120 degree bond angle

trigonal planar molecular shape

<120 degree bond angle

bent molecular shape (3 RHEDS)

109.5 degree bond angle

tetrahedral molecular shape

<109.5 degree bond angle

trigonal pyramidal molecular shape

«109.5 degree bond angle

bent molecular shape (4 RHEDS)

more lone pairs creates

greater distortion and smaller bond angles