Topic 1

Front 1

Z

Back 1

Atomic number- # of protons in the nucleus

Front 2

A

Back 2

Mass number- total # of protons and neutrons

Front 3

Isotopes

Back 3

Atoms of the same atomic number but different mass number

Front 4

Nuclear model-

Back 4

An atom of atomic number Z consists of a nucleus of charge +Ze surrounded by electrons each of charge -e

Front 5

e

Back 5

Elementary charge = 1.6022 x 10^-19 C

Front 6

c

Back 6

Speed of light = 2.998 x 10^8m/s

Front 7

h

Back 7

Planck’s constant = 6.626 x 10^-34 Js

Front 8

NA

Back 8

Avogadro’s number = 6.022 x 10^23 mol^-1

Front 9

k

Back 9

Bolzmann’s constant = 1.3806 x 10^-23 J/K

Front 10

R=NA k

Back 10

Gas constant= 8.3145 J/(mol K)

Front 11

F = NA e

Back 11

Faraday’s constant = 9.6485 x 10^4 C/mol

Front 12

Atomic orbitals

Back 12

Regions of space where electrons are most likely to be found, with no more than two electrons in any one orbital.

atomic orbitals are arranged in shells around the nucleus, each shell is characterized by its principle quantum number, n = 1, 2, ...

a shell consists of n^2 individual orbitals, which are grouped together into n subshells; these subshells, and the orbitals they contain, are denoted s, p, d, and f.

Front 13

Periodic table

Back 13

The vertical columns of the table are called groups and are numbered from 1-18. Successive rows of the the table are called periods, the number of the period being equal to the principle quantum number of the valence shell, the outermost shell.

The periodic table is divided into s, p, d, and f blocks. The d block (groups 3-11) are known as transition metals; the f block (lanthanides period 6 and actinides period 7) are known as inner transition metals; s block are groups 1-2; p block groups 13-18.

Front 14

Common group names

Back 14

Group 1 = Alkali metals

Group 2 = alkaline earth metals

Group 17 = halogens

Group 18 = Noble gases

Broadly speaking, the elements towards the left of the periodic table are metals and those toward the right are non-metals; the two classes of substances meet at a diagonal line running from boron to polonium, which constitute the metalloids, with properties intermediate between those of metals and non-metals.

Front 15

Anion

Back 15

When an atom gains one or more electrons it becomes negatively charged

Front 16

Cation

Back 16

When an atom loses one or more electrons it becomes positively charged

Front 17

Oxidation number

Back 17

The charge number of an ion. ie. Mg^2+ has two fewer electrons than protons. O^2- has two more electrons than protons.

Front 18

Chemical bond

Back 18

Link between atoms

Front 19

Ionic bonds

Back 19

Typically, but far from universally, contain a metallic element and consist of cations and anions in a crystalline array. The bond does not just exist between two individual ions. For this reason, the smallest unit of an ionic compound is called a formula unit. NaCl consist of Na^+ and Cl^- the formula unit is sodium chloride because the crystalline structure exist in a one to one ratio

Front 20

Covalent bonds

Back 20

Consist of discrete molecules. The bonds between atoms consist of shared electrons

Front 21

Hypervalent

Back 21

Atoms of period 3 and later can accommodate more than eight electrons in their valence shell.

Front 22

Resonance VS

Back 22

When more than one Lewis structure can be written for a molecule, a blending of the structures may occur and distribute multiple-bond character over the molecule.

Front 23

VSEPR

Back 23

Valence-shell electron pair repulsion theory. The regions of high electron density, as represented by bonds- whether single or multiple- and lone pairs, take up orientation around the central atom that maximize their separations. Lone pairs are assumed to repel bonding pairs more strongly than bonding pairs repel each other.

Hint 23

Front 24

Polar bonds

Back 24

Unequal sharing of electron pairs in a covalent bond results in one atom having a partial positive charge and the other atom a partial negative charge. The juxtaposition of equal and opposite partial charges constitutes an electric dipole

Front 25

Electronegativity

Back 25

The ability of an atom to attract electrons to itself

Front 26

Properties of bulk matter

Back 26

Mass: measured in kg; 1kg = 2.205 lbs

Volume: 1m^3: 1dm^3 = 1L

Amount of substance: mole; 1mole = 6.022 x 10^23 (the number of carbon atoms in exactly 12g of carbon-12)

Front 27

Extensive property

Back 27

Property that depends on the amount of substance present in the sample. (Volume, mass)

Front 28

Intensive property

Back 28

A property that is independent of the amount of substance. (Color, density, melting point, boiling point, specific heat, etc)

Front 29

Pressure

Back 29

Force/Area: 1pascal or 1bar = 10^5 Pa or 1atm = 101325Pa

Front 30

Perfect gas

Back 30

Also called ideal gas, pV = nRT

R = gas constant 8.3145 J/(mol K)

All gases obey the perfect gas equation ever more closely as the pressure is reduced towards zero.

Front 31

Boyle’s law

Back 31

Pressure is inversely proportional to the volume

p ~ 1/V

Front 32

Charles’s law

Back 32

Pressure is proportional to temperature

p ~ T

Front 33

Avogadro’s principle

Back 33

Volume is proportional to the amount of substance

Front 34

Limiting law

Back 34

A law that becomes increasingly valid in a particular limit.

Ex: in the ideal gas equation, as the pressure is reduced to zero

Front 35

Dalton’s law

Back 35

A mixture of perfect gases behaves like a single perfect gas. The total pressure of such a mixture is the sum of the pressures to which each gas would give rise if it occupied the container alone.

p = pA + pB + ...

Each pressure can be calculated, individually, by the perfect gas equation