Chem 115 Exam 2 - Electron Configuration, Periodic Trends, Bonding

light shining on metal

when light shines at metal at specific wavelength an electron is ejected

shells in first row

1

shells in second row

2

shells in third row

3

IE on periodic table

increases to top right corner

electron affinity

increases to top right corner

electronegativitiy

increases to top right corner

atomic radius

increases to bottom left corner

non metal characteristics on periodic table

increases diagonally to top right corner

metal characteristics on periodic table

increases diagonally to bottom left corner

dimagnetic

electrons are only paired in orbitals, they are not attracted by magnetic field

paramagnetic

one or more orbits with unpaired electrons, weakly attracted by magnetic field

n (principle)

size given by row on periodic table

lower = smaller orbit and energy

l (angular)

shape given by s p d and f

s orbitals

far left section on periodic table

2 electrons

l = 0

p orbitals

far right side of periodic table

6 electrons

l = 1

d orbitals

center section of periodic table

10 electrons

l = 2

f orbitals

separate section on periodic table

14 electrons

l = 3

ml (magnetic)

orientation in space or orbitals

corresponds to l

l = 1 : ml = (-1,0,1)

ms (spin)

two directions possible (arrow up or arrow down)

sub level filling order

diagonal starting with s1 → s2 → 2p → 3s

final electron level shows…

row section ^ number in section

metal characteristics

form cations

basic

reductive → electrons gained

high melting point

good conductor

nonmetal characteristics

form anions

acidic

oxidation → electrons lost

low melting point

bad conductors

bond strength

increases up columns

ionic bond characteristics

different electronegativities

between metal and nonmetal

nonpolar

covalent bond characteristics

similar electronegativies

between 2 non metals

polar

bent shape

2 lone pairs and 2 bonds

valance electrons on periodic table

increases left to right skipping center section

lattice energy

given steps work backwards, then total each delta H (MIND THE LEAD COEFFICIENTS)

enthalpy

Hf = Hreactant - Hproduct

lattice energy increases with

small radius

lattice energy decreases with

large radius

stable electron configuration

full or half filled sections

noble gases on periodic table

far right column

isoelectronic

same charge as a noble gas

isoelectronic series

in order from atom increasing charge, to noble gas, to atom decreasing charge

outer electrons

furthest out shell with the highest n number

valance electrons

last set of electrons in diagonal structure

low bond dissociation

low electronegativity

high bond dissociation

high electronegativity