Chemistry - formation of ions/ionic/metallic/covalent bonding

How are ions formed?

When atoms lose or gain electrons to obtain a full valence shell.

what type of ions are formed in groups 1,2,3?

cations/positive

what type of ions are formed in groups 4,5,6

anions/negative

If forming positive ions do they lose or gain electrons.

lose

Why do the electrons of the valence shell transfer

they are less attracted to the nucleus

What does it mean when the ions are isoelectronic with the next noble gas

they have the same electron configuration

naming regative ions

-ide

Naming positive ions

element name + ion

What is ionic bonding?

The electrostatic attraction between oppositely charged ions

What type of ion are metals?

cations

What are polyatomic ions?

ions that are made of more than one atom

hydroxide ion

OH-

nitrate

NO3-

sulfate

SO4 2-

carbonate

CO3 2-

ammonium

NH4+

Copper (III)

Cu2+

Iron (II)

Fe2+

Iron III

Fe3+

Lead II

Pb2+

Zinc

Zn2+

Silver

Ag+

what is the structure of cations and anions

giant lattace of altemating

Why do ionic compounds have high melting and boiling points?

It takes a lot of energy to break the electrostatic attraction

the greater the magnitude of the charge on the ion

the stronger the ionic melting point

When do ionic compounds conduct electricity?

when melted or (aqueous) dissolved in water

Ions are what

brittle

what is the structure of metallic bonding

lattice of metal cations surrounded by a sea of delocalized electrons.

what is a metallic bond

electrostatic attraction between metal cations and delocalised electrons

what are the delocalized electrons?

The "sea" of valence shell electrons of a metal (free to move)

What does delocalised mean?

not attached to a specific ion/free to move around metallic structure

when can metals conduct electricity

in any state

Why can metals conduct heat?

The delocalised electrons can quickly carry thermal energy through the structure.

Why are metals maleable/ductile

layers of cations can slide over each other when force is applied.

what is covalent bonding?

The electrostatic attraction between valence electrons and positive nuclei of non-metal atoms.

what is the difference between discrete and continuous.

Discrete - you can tell when structure ends. Continuous- structure repeats and is connected.

Can covalent molecules conduct electricity

no - they are fixed and cannot move

Are the melting and boiling points of covalent (simple molecular) compounds high or low and why?

low - the covalent bonds need lots of energy to break but the intermolecular/attractive forces break.

removing attractive forces causes the molecules to do what

spread

As the covalent bonds get larger the

strength of the molecular forces increase - higher melting and boiling points.

allotrope meaning

substances containing only one type of atom arranged in different structures.

non-metal atoms share electrons but

form lattices

Does diamond have a high or low melting and boiling point?

high - no intermolecular forces and the covalent bonds need energy to be broken.

Is diamond hard or soft?

hard - pyramid/tetrandel structure resists force; strong covalent bonds.

Does diamond conduct electricity?

No because it has no free electrons or ions

Does graphite have a high or low melting and boiling point?

high but not as high as diamond - low energy needed to break intermolecular forces but high energy to break covalent bonds.

Is graphite hard or soft?

soft - intermolecular layers are weak - layers can slide over each other easily

Can graphite conduct electricity?

Yes, because it has a delocalised electron.

Does Fullerene have a high or low melting point?

m.p lowers than diamond and graphite. Molecules of c60 are connected by weak intermolecular forces that don't need a lot of energy to break.

Is fullerene soft or hard?

soft - held together by weak intermolecular forces.

Does fullerene conduct electricity?

no - each c atom is bonded to 3 others but spare electrons cannot be delocalized between molecules.