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Chemistry > Bonding, structure and properties of matter > Flashcards

Bonding, structure and properties of matter Flashcards

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1
Q

Describe ionic bonds (3 points)

A

-Takes place when metals and non-metals react by transferring electrons
-The atoms involved are oppositely charged particles (known as ions) in which electron transfer occurs
-The opposite charges attract through electrostatic forces

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2
Q

How are covalent bonds formed

A

non-metal atoms share pairs of electrons between each other

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3
Q

When are metallic bonds formed?

A

This type of bonding occurs in metals and metal alloys (mixtures of metals)

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4
Q

What is an ion?

A

An ion is an electrically charged atom or group of atoms formed by the loss or gain of electrons

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5
Q

Why do atoms lose or gain electrons?

A

To be stable and have a full outer shell of electrons

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6
Q

What are negative ions called?

A

Anions

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7
Q

What are positive ions called?

A

Cations

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8
Q

What ions do metals form?

A

Cations(+)

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9
Q

What ions do non-metals form?

A

Anions(-)

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10
Q

How are ionic compounds held together?

A

The positive and negative charges are held together by the strong electrostatic forces of attraction between oppositely charged ions

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11
Q

In what direction do electrostatic forces form?

A

In all directions

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12
Q

Describe the structure of an ionic compound?

A

The lattices formed by ionic compounds consist of a regular arrangement of alternating positive and negative ions in which the ions are tightly packed together

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13
Q

What allows solid ionic compounds to form regular shapes?

A

The lattice arrangement exists in three dimensions which allows solid ionic compounds to form regular shapes

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14
Q

Are covalent bonds strong?

A

Covalent bonds between atoms are very strong

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15
Q

When are molecules formed?

A

When two or more atoms are covalently bonded together, they form ‘molecules’

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16
Q

Describe inter molecular forces in a covalent molecule?

A

Weak inter molecular forces exist between individual molecules

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17
Q

Do simple covalent molecules conduct electricity? Why?

A

Simple covalent molecules do not conduct electricity as they do not contain free electrons

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18
Q

What is the difference between bonding in ionic vs covalent bonding?

A

In ionic bonds, electrons are completely transferred from one atom to another. In covalent bonding, electrons are shared between two atoms.

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19
Q

What are small covalent structures called?

A

These small molecules are known as simple covalent molecules

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20
Q

What are polymers?

A

Giant covalent structures

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21
Q

Name three substances with giant covalent structures

A

-Graphite
-Diamond
-Silicon dioxide

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22
Q

2 pros of dot and cross diagrams

A

-shows the transfer of electrons
-shows which atom the electrons are coming from

23
Q

2 cons of dot and cross diagrams

A

-Fails to illustrate the 3D arrangements of the atoms and electron shells
-Doesn’t indicate the relative sizes of the atoms

24
Q

2 pros of ball and stick model

A

-Useful for illustrating the arrangement of atoms in 3D space
-Especially useful for visualizing the shape of a molecule

25
Q

2 cons of ball and stick model

A

-Fails at indicating the movement of electrons
-The atoms are placed far apart from each other, which in reality is not the case as the gaps between atoms are much smaller

26
Q

2 pros of 2D model

A

-Displayed formulae are 2D representations and are basically simpler versions of the ball and stick model
-Adequately indicate what atoms are in a molecule and how they are connected

27
Q

2 cons of 2D model

A

-Fail to illustrate the relative sizes of the atoms and bonds
-Cannot give you an idea of the shape of a molecule and what it looks like in 3D space

28
Q

Describe the arrangement of atoms in pure metals

A

Metals consist of giant structures of atoms arranged in a regular pattern in a lattice

29
Q

Are delocalised electrons transferred in metals

A

Delocalised electrons are not transferred as in ionic bonding, they are merely moving freely in the spaces in-between the nuclei of metal atoms.

30
Q

What is an inter-conversion of state?

A

When matter changes from one state to another due to changes in temperature or pressure, the change is called an inter-conversion of state

31
Q

Is an inter-conversion of state a physical or chemical change?

A

It is a physical change involving changes in the forces between the particles of the substances, the particles themselves remain the same, as do the chemical properties of the substance

32
Q

What is sublimation?

A

gas to solid

33
Q

What does particle theory explain?

A

Particle theory explains how matter changes state depending on the energy and forces present between the particles in the substance

34
Q

What does the amount of energy needed to change from a solid to a liquid and from a liquid to a gas depend on?

A

The amount of energy needed to change from a solid to a liquid and from a liquid to a gas depends on the relative strength of the forces acting between the particles

35
Q

Why is the amount of energy needed to change state for each substance different?

A

Since each substance contains different particles, then the amount of energy needed to induce a change of state is different for each individual substance

36
Q

Why do particles gain more energy when they are heated?

A

When substances are heated, the particles absorb thermal energy which is converted into kinetic energy

37
Q

How does melting occur?

A

Heating a solid causes its particles to vibrate more and as the temperature increases, they vibrate so much that the solid expands until the bonds break and the solid melts

38
Q

How does Boiling occur

A

On further heating, the now liquid substance expands more and some particles at the surface gain sufficient energy to overcome the intermolecular forces and evaporate

39
Q

What is latent heat?

A

While changing state, the temperature of the substance remains the same as the heat energy goes into breaking the bonds between the particles

40
Q

Which diagram can be used to summarise latent heat?

A

Heating and cooling curve

41
Q

Limitations of the particle model?(3)

A

-considers all particles to be solid,inelastic regardless of state
-It doesn’t consider the difference caused by different particles, such as atoms, ions or molecules or mixtures of all three
-The theory also fails to consider the intermolecular forces that exist between different particles in different substances

42
Q

What does ⇌ show?

A

reversible

43
Q

Physical properties of ionic compounds?(3)

A

-Soluble in water
-hard + brittle
-good insulators

44
Q

Why do ionic compounds have high MP & BP points?

A

Ionic substances have high melting and boiling points due to the presence of strong electrostatic forces acting between the oppositely charged ions

45
Q

When do ionic compounds conduct electricity?

A

Molten or liquid form

46
Q

Why can’t ionic compounds conduct electricity when solid?

A

They cannot conduct electricity in the solid state as the ions are in fixed positions within the lattice and are unable to move

47
Q

Do small covalent molecules have a high or low BP?

A

Low boiling points due to weak intermolecular forces that require little energy to overcome

48
Q

Can covalent compounds dissolve in water?

A

Most covalent compounds are insoluble in water as they tend to be non-polar but can dissolve in organic solvents

49
Q

Can covalent molecules conduct electricity?

A

They are poor conductors of electricity as there are no free ions or electrons to carry the charge.

50
Q

Are covalent molecules good insulators?

A

Most covalent compounds do not conduct at all in the solid state and are thus insulators

51
Q

Where are intermolecular forces found?

A

Between molecules

52
Q

Relationship between size of molecule and strength of intermolecular forces?

A

As the molecule increases in size the strength of the intermolecular forces increases

53
Q

GOT UP to polymers

A

Chemistry (4 decks)

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