Chemistry terms IB SL

Multivalent

elements that can form ions with different charges

Volatility

vapourizes easily

Malleability

ability of metals to be hammered into shapes without breraking

Isomer

Organic compounds with the same formula but different arrangement

Subscript

Number of atoms

Coefficient

Multiplier

Ar

Average relative mass

Ar =

sum of isotopes (mass number x percent abundance /100)

Group One Metals + H2O =

H2 gas and metal hydroxide aqueous

free radical

atom with an unpaired electron

As strength of IMFS increases

Melting point increases and boiling point increases

As strength of IMFs decreases

Melting point decreases and boiling point decreases

Zeff =

number of protons - number of core electroms

Boiling point of branched

Lower, weaker

Boiling point of straight

Higher, stronger

Boiling point with more carbons in chain

Higher, stronger

Combustion reaction produces

CO2, CO, or C and H2O

M

molar mass

m

mass

N

number of particles

n

moles

Volume and moles equation

V1/n1=V2/n2

Pressure and Volume equation

P1V1=P2V2

Volume and temperature equation

V1/T1=V2/T2

Combined gas law

P1V1/T1=P2V2/T2

In pv=nrt, p needs to be in

Pascals

In pv=nrt, v needs to be in

m3

in pv=nrt, n needs to be in

mols

in pv=nrt, t needs to be in

Kelvins

Breaking bonds

endothermic, +

Forming bonds

exothermic, -

More stable

lower energy

1 atm =

101 kpa

using enthalpies of formations

products - reactants

using enthalpies of combustion

reactants - products

using bond enthalpies

reactants - products

3 points of collision theory

1) 2 particles must collide

2) They must collide with correct orientation

3) They must have enough energy to react

Smaller molecules

react faster, lower molar mass

Adding temperature makes the maxwell boldsman curve

flatter and ending higher

Lowering temperature makes the maxwell boldsman curve

Sharper and ending lower

first 2 groups

s energy level

last 6 groups

p energy level

middle groups

d energy level

what does a maxwell boldsman show

the proportions of kinetic energies of a sample of particles

pressure ______ rate

increases

temperature _____ rate

increases

concentration _____ rate

increases

particle size ______ rate

decreases

volume ______ rate

decreases

ionic bonding is due to

electrostatic attraction between oppositely charged ions

binary acid ends with

hydro ____ -ic acid

oxyacid ends with

-ate

nucleophile

electron pair donor

hydrated ionic compound is a

crystal

electrophile

electron pair acceptor

initiation

halogen free radical is made

propogation

hydrogen leaves alkane, goes to halogen free radical

methyl free radical gains halogen

termination

2 free radicals reacting to form a covalent species

lattice

repeating arrangement of empirical formula

certain ions have stronger lattice enthalpy because of

smaller radius

what makes central atoms have less domains

double bonds

Equilibrium

Where the rate of forward and reverse reactions are equal in a closed system

Equilibrium only applies to

aqueous and gas

Large Kc (more what) (what is favoured)

more products than reactants, forward reaction is favoured

Small Kc (more what) (what is favoured)

more reactants than products, reverse reaction is favoured

Kc > 1

product favored

homolytic fission results in

two free radicals

heterolytic fission results in

a cation and an anion

Metals

malleable, high melting point, high boiling point, high electrical and thermal conductivity

Non metals

brittle, low melting point, low boiling point, low electrical and thermal conductivity

amphoteric

can act as acid or base

increase in temp shifts equilibrium to the side of

endothermic reaction

decrease in temp shifts equilibrium to the side of

exothermic reaction

Smaller radius

higher force of attraction between nucleus and electrons

higher electron affinity means

it's easier to gain an electron

More valence electrons has ____ radius

smaller

Ionization energy

The amount of energy required to remove one mole of electrons from one mole of gaseous atoms

As radius ___, ionization energy ____

increases, decreases

As nuclear charge ____, radius ____

increases, decreases

What is responsible for radius, ionization energy, electron affinity and electronegativity?

Force of attraction between nucleus and valence electrons

_____ ionization energy, electron affinity and electronegativity increase

across a period

____ ionization energy, electron affinity, and electronegativity decrease

down a group

H

heat transferred at constant pressure

q

enthalpy change

acid and base react to form a

salt and water

[OH] from POH

10 to the power of -pOH

[H] from PH

10 to the power of -pH

strong acids

HCl, HBr, HNO3, H2SO4

strong bases

group one hydroxides

Pure water has a pH of

7

Voltaic cell anode is

negative

Voltaic cell cathode is

positive

Electrolytic cell anode is

positive

Electrolytic cell cathode is

negative

Voltaic cell

spontaneous chemical reaction causes a flow of electrons

Electrolytic cell

A non-spontaneous cell driven by an external voltage.

Most reactive

top half right side, bottom half left side