Atom Structure, Balancing Equations, Acids

Chemistry Revision Pre-IB T1

Atom

Smallest part of a chemical element

groups

column (vertical)

periods

rows (horizontal)

metaloid

properties of metals and non-metals

isotope

more neurons than protons

diatomic elements

H2, N2, F2, O2, I2, Cl2, Br2 (Have No Fear Of Ice Cold Beer)

(most are halogens except astatine).

compound

2+ different elements chemically bonded

molecule

2 or more same element

atom

smallest particle/unit of a chemical element

molecule properties

discrete (isolated) in connectedness:

e.g. crystalline organised arrangement

relative mass

add both elements together

stoichiometric ratio

ratio of coefficients

balancing equations layout

reactant/s yields product/s

Law of Conservation of Mass

mass is neither created nor destroyed

state symbols

solid (s), liquid (l), gas (g), and aqueous (aq)

Ionic Compounds

electrostatic attraction between oppositely charged ions

stable octet / noble gas configuration

a stable electron configuration consisting of 8 valence electrons

cations

+ charged ions

anions

- charged ions

ion

a molecule with a net electrical charge

ionic compound properties

-High Melting / Boiling points

-When solid it can't conduct electricity

-Dissolve easily in water

-hard, brittle, lattice structure, crystalline solids

naming ionic compounds

metal+non-metal(ide)

Polyatomic Ion

A charged group of covalently bonded atoms

Isoelectronic species

Atoms or ions with the same electron configuration.

How to draw a polyatomic ion

if not lewis structure, remove the silly bonding lines)

Solubility

if soluble in water, will form an aqueous solution

if not, stays the same state

net ionic vs ionic equation

net ionic equation - without spectator ions

ionic equation - every individual w/ charge

covalent bonding

sharing electrons between 2 non metals

ionic bonding

linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound

non-bonding pairs/lone pairs

not involved in forming the bond in the valence shell

core electrons

The electrons that are not in the outermost shell of an atom.

covalent bond properties

-low melting/boiling points

-bad electricity conductivity

-single double or triple bonds

-weaker bonding

naming covalent compounds

mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca

lewis dot diagram

only represents valence shell bonding electrons

-usually covalent compounds

metallic bonding

The electrostatic attraction between metal cations and delocalised electrons.

metallic bonding properties

1) lattice structure

2) Delocalised electrons

3) Strong forces of ELECTROSTATIC ATTRACTION between positive metal ions and negative electrons

4) Solid at room temperature

5) High melting and boiling points

6) bright lustre

7) hardness

8) resonant sounds

9) excellent conductors

metals

electropositive elements with relatively low ionisation energy (not much energy to remove an electron)

lattice

regular repeating structure

alloy

A mixture of two or more metals

Quantitative

numerical data and allows for math analysis

-trends, patterns, relationships, limitations and uncertainty

Qualitative

descriptive data

-colour, chaage, state, temp, length/time of reaction

-descriptions on before, during and after

-can be recorded

Acid

a compound in which one or more H+ ions are bonded to a negative ion

ide - hydro___ic acid

ate - ____ic acid

ite - ____ous acid