Chem 115 Final (Exams 1-3 and New Material)

number of moles

grams / molar mass

molarity (M)

number of moles / volume (L)

limiting reagent

least number of moles AFTER dividing by lead coefficients

dilution

M1V1 = M2V2

% error

((experimental - actual) / actual) * 100

cation (+)

less electrons

anion (-)

more electrons

law of conservation of mass

total mass doesn’t change during a reaction

what does an acid produce?

H+

what does a base produce?

OH-

positive delta H

endothermic (heat gained)

negative delta H

exothermic (heat released)

delta H reaction

H product - H reaction

calculating delta H

-(heat released) / number of moles

H

E + PV

work on system

volume of gas decreases, w = +

work by system

volume of gas increases, w = -

calculating work

-P * deltaV

heat capacity

q = C * deltaT

specific heat capacity

q = m*c*deltaT

heat released

q = -

heat gained

q = +

calculating change in energy

delta E = q + w

alpha decay

change in both atomic mass and number (top right corner on band of stability)

beta decay (negitron)

change in atomic number (+ 1) (top left above band of stability)

beta (positron)

change in atomic number (-1) (under band of stability)

electron capture

change in atomic number (-1) (under band of stability)

gamma

no change in atomic number or atomic mass

isotope model “A”

represents the atomic mass

isotope model “Z”

represents the atomic number (number of protons)

isotope model “X”

represents symbol of element

isotope model “A-Z”

number of neutrons

nucleon

number of protons and neutrons

fusion

small mass to big mass

fission

big mass to small mass

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

characteristics of a metal

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

polarity

difference in electronegativity

covalent bonding

• 2 non metals

• similar electronegativity

• e- shared

ionic bonding

• metal and nonmetal

• different electronegativity

• e- fully taken by more electronegative

metallic bonding

• 2 metals

• conductive

electron group arrangements

• linear

• trigonal planar

• tetrahedral

name this structure and its angles

• linear

• 180

name this structure and its angles

• trigonal planar

• 120

name this structure and its angles

• bent

• < 120

name this structure and its angles

• tetrahedral

• 109.5

name this structure and its angles

• trigonal pyramidal

• <109.5

name this structure and its angles

• bent

• < 109.5

formal charge formula

valency - (#sticks around atom + #dots around atom)

when can elements overfill their octet?

when they’re past phosphorus

single bonds

• 1 sigma

• weak

• free rotation

double bonds

• 1 sigma 1 pi

• no free rotation

triple bonds

• 1 sigma 2 pi

• no free rotation

• strong

prefix for 1

meth-

prefix for 2

eth-

prefix for 3

prop-

prefix for 4

but-

prefix for 5

pent-

prefix for 6

hex-

prefix for 7

hept-

prefix for 8

oct-