inorganic chem

neutrons

have no charge, have a mass, in nucleus

protons

positive charge , same mass os neutrons, found in nucleus

electrons

negative charge, mass of 1/1836 that of protons, found in spac3 surrounding nucleus

atomic number(z)

number of protons in the nucleus

mass number (a)

number of protons and neutrons in the nucleus, the larger number electron configuratione

election configuration

the distribution of electrons in an atom's orbitals, indicating how they are arranged. controls the chemical and physical properties.

metals

shiny, malleable, conduct electricity. eg AI, FE

non metals

not malleable or ductile, don’t conduct electricity, eg C, S

metalloids

have the appearance and some physical properties of metals but behave chemically like non-metals, eg Si

s orbital

shaped like a sphere, one s orbital within the s sub shell, can hold 2 electrons.

p orbital

have two lobes, shaped like a dumbbell, 3 p orbitals of equal energy.

degenerate orbitals

election orbitals with the same energy orbitals

Hund’s rule

whenever 2 or more orbital of equal energy are available the electrons will occupy them singly before pairing up.

pauli’s electron principle

each orbital can hold one pair of electrons; but the electrons will have opposite spins.

alkali metals

group one, soft silvery metals, melt at low temps, single electron outer shell

alkaline metals

group 2, soft metals, found in nature of oxides, used in radiation therapy, 2 electrons in outer shell

halogens

group 7, very reactive, nonmetals, 7 electrons in outer shell

noble gases

group 8, colourless orderless gases, full outer shell, unreactive/stable

transition elements

d-block, can for compound in several oxidTION STATED

chemical bond

a connection between a pair of atoms formed by an exchange of their outermost electrons.

ionic bond

is formed by the attraction of oppositely charged ions, the bonding electrons localise around the negative ion.

covalent bond

formed by the sharing electrons between two uncharged atoms, the bonding electrons are shared between the two atoms.

molecular compounds

the atoms bonded together into molucules

ionic compounds

consist of 2 or more electrically charged ions in which the overall charge is zero.

covalent compounds

formed between atoms which differ by little(or not at all) in their tendency to lose or gain electrons(electronegativity)

ionic compounds

formed between atoms with large differences in their tendency to Gain or lose electrons

lone pair

an outer level elctron pair not involved in bonding

VSEPR

valence shell electron pair repulsion theory. it uses the electron pairs from lewis structures to predict the 3D shape of molecules

polar covalent bond

exists between two atoms of different electronegativites, the electrons are closer to the more electronegative atom, creating a dipole moment. one side more + one side more -

non polar covalent bonds

occur between two atoms of similar electronegativities, where electrons are shared equally, resulting in no dipole moment.

solubility

ability of a give substance (solute) to dissolve in a solvent, measured in terms of the maximum amount of solute dissolved at equilibrium.

theoretical yield

the amount of product formed when the limiting reagent is completely consumed

percentage yield

the actual yells of the product

precipitation reaction

occurs when two solutions of strong electrolytes are mixed

redox reaction

involve reduction or oxidation

oxidation numbers

an arbitrary system to allow us to keep track of electrons, electrons are redistributed as elements react with each other

nuclear reactions

atoms of one element typically change into atoms of another radioactive half life r

radio active half life

time taken for activity to reach half f its initial value

PET

proton emission tomography, can be used to track a substance in the body