Atomic Structure

Atomic structure & Chemical bonding

Cation

An atom or molecule with fewer electrons than protons

Isotope

An atom with more neutrons than the typical atom of the same elements

Electron Cloud

The location outside the nucleus where electrons are found

Anion

An atom or molecule with more electrons than protons

Compound

2 or more atoms chemically bonded in specific ratios

Atomic Number

The number of protons in an atom

Mass number

Total number of protons and neutrons in an atom

Mass of an electron

.0001

Group

Vertical columns of the periodic table

Period

Horizontal rows of the periodic table

How many protons in C-16 (3+)

6

How many neutrons in C-16 (3+)

10

How many electrons in C-16 (3+)

3

How many protons in N-12 (2-)

7

How many neutrons in N-12 (2-)

5

How many electrons in N-12 (2-)

9

How many electrons in N-14 (4-)

11

How many neutrons in N-20 (4-)

13

Ionic Bond (definition)

Bond formed when 1 or more electrons are transferred from one atom to another

Types of bonds

Ionic, covalent, metallic

Ionic Bond (description)

A chemical bond resulting from the attraction between oppositely charged ions

Ionic bond (types of elements)

Metals with non-metals

Ionic bond (nature of)

Electrostatic attraction

Coulombic attraction

The attraction between oppositely charged particles

Metals in ionic bonds

Few valence electrons tend to lose them, form positive ions

Non-metals in ionic bonds

Many valence electrons gain a few, form negative ions

Metallic bond (definition)

A bond formed by the attraction between positively charged metal ions and the electrons around them

Metallic bond (model)

A ‘sea of delocalised electrons’ around metal atoms

Alloy

A mixture of 2 or more elements, one of which is a metal

Ally (examples)

Sterling silver, bronze, brass and steel

Sterling silver

Alloyed with copper

Bronze

Copper alloyed with tin

Covalent bond (definition)

A chemical bond that involves sharing a pair of electrons between atoms in a molecule

Covalent bond (types of elements)

2 or more non-metals

Another term for covalent bond

Molecular bond

Single Bond

A covalent bond in which 2 atoms share 1 pair of electrons

Double bond

A covalent bond in which 2 atoms share 2 pairs of electrons

Triple bond

A covalent bond in which 2 atoms share 3 pairs of electrons

Coordinate covalent bond

A covalent bond in which one atom contributes both bonding electrons

Polar covalent bond

A covalent bond in which electrons are not shared equally

Electronegativity

The ability of an atom to attract electrons when the atom is in a compound

Diatomic molecule (definition)

A molecule that consists of 2 atoms of the same element when in the free state

Diatomic molecule (elements)

N2, O2, F2, Cl2

Octet rule

Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually 8 valence electrons

What does VSEPR stand for?

Valence shell electron pair repulsion theory

VSEPR Theory

The repulsion between electron pairs causes molecular shapes to adjust so that the valence electron pairs stay as far apart as possible

List these in order of increasing polarity HF, Hl, HBr, HCl

Hl, HBr, HCl, HF

Bond dissociation energy

Energy required to break a covalent bond, the higher the BDE, the stronger the bond