Bonding Flashcards by Benjamin Thomas

What do ionic bonds form between

A metal and a non-metal

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What is the attraction between ions called

Electrostatic attraction between the opposite charges of ions in a lattice

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What is the formula and charge of a sulphate ion

SO4 2-

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What is the formula and charge of a hydroxide ion

OH 1-

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What is the formula and charge of a nitrate ion

NO3 1-

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What is the formula and charge of a carbonate ion

CO3 2-

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What is the formula and charge of a ammonium ion

NH4 1+

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Properties of ionic compounds

Solid at room temperature
Giant structures
High melting points
Conduct electricity when molten / dissolved

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What does a covalent bond contain

A shared pair of electrons

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What is another name for a dative bond

A coordinate bond

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What is a dative bond

Contains a shared pair of electrons with both electrons supplied by 1 atom

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How are dative bonds represented

An arrow

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Why do metals conduct electricity

They have delocalised electrons

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What does the strength of a metallic bond depend on

Number of delocalised electrons
Size of the ions

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What are the 4 types of crystal structure

Molecular
Macromolecular
Ionic
Metallic

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What is the structure of diamond

Consists of pure carbon
4 covalent bonds
Bond angles of 109.5

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What is the structure of graphite

Consist of pure carbon
Has 3 strong covalent bonds and VDW’s
120 bond angles
Has delocalised electrons so can conduct electricity

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Why do metals have high boiling points

They have giant structures. Large amounts of energy are needed to overcome the metallic bonds

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What are bonding pairs of electrons

2 electrons shared between atoms

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What are lone pairs of electrons

A pair of valence electrons (electrons on the outer shell) that are not shared with another atom

Why do pairs of electrons position themselves as far from each other

To minimise repulsion

What is the order of repulsion strength from highest to lowest

Lone pair-lone pair
Lone pair-bond pair
Bond pair-bond pair

How does a lone pair of electrons effect bond angles

A lone pair will push bonding pairs together

What is a molecules shape with 2 bonding electron pairs and what are the bond angles

Linear
180

What is a molecules shape with 3 bonding electron pairs and what are the bond angles

Trigonal planar 120

What is a molecules shape with 4 bonding electron pairs and what are the bond angles

Tetrahedral 109.5

What is a molecules shape with 5 bonding electron pairs and what are the bond angles

Trigonal bipyramidal 120 90

What is a molecules shape with 6 bonding electron pairs and what are the bond angles

Octahedral 90

What is a molecules shape with 3 bonding electron pairs and 1 lone pair. What are the bond angles

Pyramidal 107

What is a molecules shape with 2 bonding electron pairs and 1 lone pair. What are the bond angles

V-shaped 117.5

What is a molecules shape with 4 bonding electron pairs and 2 lone pair. What are the bond angles

Square planar 90

How do you work out number of unbonded electron pairs

Group number - (Number of atoms bonded + charge) /2

What is electronegativity

The power of an atom to attract a bonding pair of electrons towards itself **in a covalent bond**

What does electronegativity depend on

Nuclear charge (number of protons in the nucleus) Distance between nucleus and outer shell The shielding of the nuclear charge

How does the symmetry of a covalent bond between 2 atoms with different electronegativities change

The bond would be drawn towards the more electronegative atom

What does an unsymmetrical covalent bond cause

A polar bond which can lead to a permanent dipole being formed

What are the 3 types of intermolecular force

VDW forces Dipole-dipole forces Hydrogen bonding

What do VDW forces act between

All atoms and molecules

What do dipole-dipole forces act between

Act between molecules with polar bonds

What do Hydrogen bonds form between

Only between h and fluorine, oxygen or nitrogen (FON)

How do VDW forces form

At any one time in a covalent bond, some electrons may happen to be closer to one atom. This will induce a temporary dipole. This then affects neighbouring atoms so they are attracted to each other for a short space of time

What is the order of strength of intermolecular forces

Hydrogen bonding Dipole dipole bonding VDW's

Why are hydrogen bonds important in ice

When water freezes, all H bonds fix the molecules in a stable position. These molecules are further away from each other than liquid water do ice is less dense. This allows fish to survive etc

Give an example of a bond with multiple shared pair of electrons

N≡N

How are metals bonded

Metallic bonding involves attraction between delocalised electrons and positive ions arranged in a lattice

What type of structure is ice

Ice is a molecular crystal that is connected by hydrogen bonds

What type of crystal is iodine

Molecular covalent crystal

What type of crystal is sodium chloride?

An ionic salt Crystal lattice

What type of crystal is magnesium?

Giant metallic lattice