Chem Exam 2 (Ch 3.11-12, 4, 5)

1st ionization energy

energy cost to remove the first electron from an atom

what is the trend for ionization energy

from right to left; down to up

electron affinity

the amount of energy released when an atom gains an electron

high electron affinities ___ additional electrons

attract

ionic bonds are between ___ and ___

cation (metal); anion (nonmetal)

covalent bonds are between ___ and ___

nonmetals; nonmetals

___ bonds share the electrons

covalent

___ bonds send the electron from metal to nonmetals

ionic

metallic bonds

communal sharing of electrons between metals

electronegativity

how strongly an atom pulls on electrons in covalent bonds

in ionic compounds there’s a ___ EN difference

large

nonpolar means that the electrons are ___ shared

equally

polar means the electrons are ___ shared

unequally

water is ___

nonpolaro

octet rule

elements want a full shell of 8 electrons

formal charge formula

valence - # of lone pair electrons - # of bonds

bond dissociation energy

energy needed to break bond exactly in half

the shorter the bond the ___

stronger

location of hypervalent elements

3p row or lower

elements that are okay with incomplete octets

boron, aluminum, and galium

what does it mean to be a free radical

the molecule has an odd number of electrons

lattice energy

energy change when atoms make ionic bonds

trends in lattice energy

• as distance goes up, lattice energy goes down

• charge goes up, lattice energy goes up

what’s used to predict a molecule’s geometrics

VSEPR

what are the electron groups

lone pairs and single/double/triple bonds

steric number

number of electron groups

the name for two electron groups (ideal angle)

linear (180)

the name for three electron groups (ideal angle)

trigonal plane (120)

the name for four electron groups (ideal angle)

tetrahedral (109.5)

the name for 5 electron groups (ideal angle)

trigonal bipyramidal (90, 120)

the name for six electron groups (ideal angle)

octahedral (90)

strength of repulsion rankings

lone pair > triple bond > double bond > single bond

bond polarity

electronegativity

molecular polarity

ALL bond polarities

Kr

Krypton

Xe

xenon

Rn

radon

Se

selenium

P

phosphorous

As

arsenic

Si

silicon

Sn

tin

Pb

lead

Fe

iron

Ni

nickel

Mo

molybdenum

Zn

zinc

CN^-

cyanide ion

NO₃^-

nitrate ion

PO₃^-3

phosphate ion

SO₄^-2

sulfate ion

CO₃^-2

carbonate ion

NH₄⁺

ammonium ion

Pb⁺²

lead (ll) ion

Pb⁺⁴

lead (lV) ion

Fe⁺²

iron (ll) ion

Fe⁺³

iron (lll) ion

Cu⁺

copper (l) ion

Cu⁺²

copper (ll) ion

Zn⁺²

zinc ion

Ag⁺

silver ion

Au⁺

gold (l) ion

Au⁺³

gold (lll) ion

H₂SO₄

sulfuric acid

H₃PO₄

phosphoric acid

HNO₃

nitric acid

H₂CO₃

carbonic acid

HF

hydrofluoric acid

HCl

hydrochloric acid

HBr

hydrobromic acid

HI

hydroiodic acid

___ is the most reactive binary acid

HI

binary acid

an acid with hydrogen and ONE other nonmetal element

oxyacid

contains oxygen and hydrogen; normally polyatomic

H₂SO₄

sulfuric acid

H₃PO₄

phosphoric acid

HNO₃

nitric acid

H₂CO₃

carbonic acid

H₂SO₃

sulfurous acid

H₃PO₃

phosphorous acid

HNO₂

nitrous acid

HClO₄

perchloric acid

HClO₃

chloric acid

HClO₂

chlorous acid

HClO

hypochlorous acid

VSEPR is best for showing a molecule’s ___

overall shape

Lewis Dot Structures are best for showing

valence electrons and bonds

the Valence Bond Theory shows electrons in ___

orbitals

key points of the Valence Bond Theory

1. an orbital is needed from each atom

2. covalent bonds form from orbital overlap

3. the direction of the bond is determined by the position of the orbital

hybrid orbitals

when orbitals on the central atom “combine” to change shape

what is the hybrid orbital for a tetrahedral

sp³

what is the hybrid orbital for a trigonal planar

sp²

what is the hybrid orbital for a linear

sp

what is the hybrid orbital for a trigonal pyramidal

sp³d

what is the hybrid orbital for a octahedral

sp³d²