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A substance is said to be volatile if it boils at a low temperature, changing from the liquid to the gas phase.

Substances that are gases at room temperature are extremely volatile: they have high volatility. They can only be seen as liquids when exposed to low temperatures or high pressures.

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The positive and negative ions are attracted to each other by forces known as the electrostatic force of attraction. This force that holds by the oppositely charged particles together is called the ionic bond

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The positive and negative ions are attracted to each other by forces known as the electrostatic force of attraction. This force that holds by the oppositely charged particles together is called the ionic bond

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They tend to gain electrons to form anions-negative ions

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The elements in grp 14 less likely to form ions -they share electrons to form covalent bonds

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are metals they tend to lose electrons to form cations-positive ions

The charge of the ion is the same as the group number forming it for grp 1 and 2

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group 1
alkali metals
group 2
alkali earth metals
grp 17
halogens
group 3 to 13
transition elements

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usually soluble in water
-aqueous solvent

but not in organic solvents

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non-conductors in solid state

- ions are held in fixed positions by strong ionic bonds[no free-moving ions to move around] in the giant ionic lattice structure and are not free to conduct electricity

conducts in molten and aqueous states

-presence of free-moving ions to carry electric current, can conduct electricity

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strong electrostatic forces holding together the giant lattice structure requires a large amount of energy to break apart ionic bon

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strong electrostatic forces holding together the giant lattice structure requires a large amount of energy to break apart ionic bon

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hard bc ionic bonds are strong and non-directional,

brittle bc ordered arrangement of oppositely charged ions in the giant crystal lattice can be easily dislocated when force is applied

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large amounts of energy required to overcome strong forces of attraction between oppositely charged ions in giant ionic lattice structure during a change in physical state

- solid at room temperature and pressure.[non-volatile]

- have high melting and boiling points

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- high melting and boiling points (low volatility)

- hard and brittle

- non- electrical conductors in solid state but good electrical conductors when molten or dissolved in aqueous solution ( if soluable

- usually soluble in water but insoluble in organic solvents

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- giant ionic crystal lattice structure
consisting of oppositely charged ions attracted together by ionic bonds

-naturally exist in solid state

- regular arrangement of ions throughout the whole stucture

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formed when one or more electrons are transferred from the valence shell of one atom to the valence shell of another atom for both atoms to attain an octet configuration

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electrostatic attraction between oppositely charged ions (metals and non metals)

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-shows the ratio of diff types of ions

- derived by balancing the charges on positive ions with those on negative ions (net charge = 0)

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- describe ionic bonding as the electrostatic attraction between oppositely charged ions

- describe how ions can be formed as a result of electron transfer:

-  when elements in grp 1,2 and 13 lose electrons, they form positive ions or cations

- when elements in grp 15-17 gain electrons, they form negative ions or anions

- transition elements form more than one ion

- predict whether a compound or two elements would be ionic from the position of the elements in the periodic table

- state the formula of common polyatomic ions formed by non-metals in the periods 2 and 3

- describe the lattice structure of ionic compounds

- compare and explain the properties of ionic compounds resulting from its bonding

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- state the relative masses and charges of protons, neutrons and electrons

- apply the relationship between the electron arrangement of elements and their position in the periodic table up to Z= 20

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- electronic configuration
- ionic bonding
- covalent bonding
- metallic bonding
- intermolecular forces

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- vertical column in the periodic table
- runs vertically from top to bottom
- number corresponds to number of valence electrons for groups 1 and 2

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- describe the arrangement of elements in the periodic table in order of increasing atomic number

- distinguish between the terms group and period
:

- distinguish

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- periodic table
- elements, compounds and mixtures