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Chemistry > Bonding and strucutre > Flashcards

Bonding and strucutre Flashcards

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1
Q

What are the 3 types of chemical bonds

A

Ionic
Covalent
Metallic

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2
Q

Define ionic bonding

A

The electrostatic attraction between positive and negative ions

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3
Q

Define covalent bonding

A

Electrostatic attraction between a shared pair of electrons and the nuclei

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4
Q

Define metallic bonding

A

Electrostatic attraction between the positive metal ions and the delocalised electrons

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5
Q

Why does giant ionic latices conduct when liquid but no when solid

A

Solid state the ions are in fixed positions and cannot move
When in liquid the ions are free to move and can carry charge freely

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6
Q

Why do giant ionic structures have a high boiling/melting point

A

A large amount of energy is required to overcome the electrostatic bonds

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7
Q

What types of solvents dissolve ionic lattices

A

Polar solvents

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8
Q

Why are ionic compounds soluble in water

A

Water has polar bonds
Hydrogen atoms have a + charge and oxygen has a - charge
These can attract charged ions

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9
Q

what is a lone pair

A

Electrons in the outer shell that are not involved in bonding

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10
Q

What is average bond enthalpy

A

Measure of average energy needed to break the bond

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11
Q

What is a dative covalent bond

A

A bond where both of the shared electrons are supplied by one atom

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12
Q

What are the types of covalent structures

A

Simple molecular
Giant covalent

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13
Q

Describe the bonding in simple molecular structures

A

Atoms are held by strong covalent bonds and different molecules are held by weak intermolecular forces

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14
Q

Why do simple molecular have low melting/boiling points

A

Small amounts of energy needed to overcome the intermolecular forces

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15
Q

Why do simple molecular structures not conduct electicity

A

They have no free charged particles to move

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16
Q

What solvents dissolve simple molecular substances

A

Non polar solvents

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17
Q

List 3 properties of giant covalent

A

High melting/boiling points

Non conductors

Insoluble in polar and non-polar

18
Q

How doe graphite conduct electricity

A

Delocalised electrons present between the layers are able to move freely carrying the charge

19
Q

Why do giant covalent structures have high melting/boiling points

A

Strong covalent bonds within the molecules need to be broken which requires a lot of energy

20
Q

What does the shape of the molecule depend on

A

Number of electron pair in the outer shell

Number of these electrons

21
Q

What is the shape and bond angle in a shape with 2 bonded pairs and 0 lone pairs

A

Linear
180

22
Q

What is the shape and bond angle in a shape with 3 bonding pairs and 0 lone pairs

A

Trigonal planar
120

23
Q

What is the shape and bond angle in a shape with 4 bonded pairs and 0 lone pairs

A

Tetrahedral
109.5

24
Q

What is the shape and bond angle in a shape with with 5 bonded pairs and 0 lone pairs

A

Trigonal Bipyramid
90 and 120

25
Q

What is the shape and bond angle in a shape with 6 bonded pairs and 0 lone pairs

A

Octahedral
90

26
Q

What is the shape and bond angle of a shape with 3 bonding pairs and 1 lone pair

A

Pyramidal
107

27
Q

What is the shape and bond angle in a shape with 2 bonded pairs and 2 lone pairs

A

Non Linear
104.5

28
Q

By how many degrees does each lone pair reduce the bond angle

A

2.5

29
Q

Define electronegativity

A

The ability of an atom to attract the pair of electrons in a covalent bond

30
Q

Which direction of the periodic table does electronegativity increase

A

Top right, towards fluorine

31
Q

What does non-polar in a bond mean

A

The electrons in the bond are evenly distributed

32
Q

what is the most electronegative element

A

Fluorine

33
Q

How is a polar bond formed

A

Bonding atoms have different electronegativities

34
Q

What are the types of intermolecular forces

A

Hydrogen bonding
Permanent dipole-dipole interactions
London dispersion forces

35
Q

What is the strongest type of intermolecular forces

A

Hydrogen bonding

36
Q

Describe permanent dipole dipole interactions

A

When molecules with a permanent dipole is close to other non polar molecules
It causes the non polar

37
Q

Describe London dispersion forces

A

Caused by random movements of electrons

This leads to instaneous dipoles

Instantaneous dipole induces a dipole in nearby molecules

Induced dipoles attract one another

38
Q

Are London forces greater in smaller or larger molecules

A

Larger due to more electrons

39
Q

Does boiling point increase or decrease down the noble gas group

A

Boiling point increases because the number of electrons increase, so there are stronger london dispersion forces

40
Q

Why is ice less dense than water

A

In ice water molecules are arranged in a orderly pattern. It has a open lattice with hydrogen bonds

In water the lattice is collapsed and the molecules are closer together

41
Q

Why does water have a higher boiling point than expected

A

Hydrogen bonds are stronger than other intermolecular forces, so extra strength is required to overcome the forces

Chemistry (18 decks)

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