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Prelim Chemistry > The Chemical Earth > Flashcards

The Chemical Earth Flashcards

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1
Q

What is a homogenous substance?

A

A substance that contains evenly spread components.

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2
Q

What is a heterogenous substance?

A

A substance that contains unevenly spread components.

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3
Q

What is a pure substance?

A

A substance that only contains one compound.

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4
Q

What is a mixture?

A

A substance that contains several compounds.

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5
Q

What is the difference between a compound and an element?

A

A compound can be decomposed into other substances but an element can not.

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6
Q

What does filtration separate?

A

A liquid and an undissolved solid.

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7
Q

What is sedimentation, and what does it separate?

A

Waiting for sediment to settle to the bottom of a glass over time.
It separates an undissolved solid and a liquid.

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8
Q

What does distillation separate?

A

Liquids with different boiling points.

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9
Q

What is the difference between evaporation and distillation?

A

In evaporation, the liquid that evaporates is not collected.

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10
Q

What is decantation?

A

Slowly pouring a liquid off the top of a solid.

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11
Q

What does crystallisation separate?

A

Components with different solubilities.

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12
Q

What does centrifugation separate?

A

Components with different densities or in different states.

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13
Q

Name a mixture in the biosphere, and state an element and a compound found within it.

A

Mixture - Soil
Elements - Iron, Oxygen, Nitrogen
Compounds - Water

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14
Q

Name a mixture in the lithosphere, and state an element and a compound found within it.

A

Mixture - Rock
Elements - Gold, Silver
Compounds - Ore

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15
Q

Name a mixture in the hydrosphere, and state an element and a compound found within it.

A

Mixture - Sea Water
Elements - Oxygen, Nitrogen
Compounds - Water, Sodium Chloride

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16
Q

Name a mixture in the atmosphere, and state an element and a compound found within it.

A

Mixture - Air
Elements - Oxygen, Nitrogen, Argon
Compounds - Water, Carbon Dioxide

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17
Q

What is the relationship between a solute and a solvent?

A

A solute is dissolved in a solvent in solution.

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17
Q

When compounds contain oxygen and another element, their suffix changes to what?

A

‘-ite’ if it is the variant with the least oxygen

‘-ate’ if it is the variant with the most oxygen

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18
Q

If extra hydrogen is added to a compound, what about its name changes?

A

‘bi-‘ is added to the second term.

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19
Q

What is the relationship between the reactivity of an element and how likely it is to be found uncombined in nature.

A

The less reactive an element the more likely it is that it will be found uncombined in nature.

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20
Q

What is the name of the following compound?

KHCO3

A

Potassium Bicarbonate

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21
Q

Define a physical property and give four examples of physical properties.

A

A physical property can be examined without a chemical change in the substance.

Eg Boiling Point, Colour, Conductivity, Hardness and Malleability

22
Q

Define a chemical property and give two examples of chemical properties.

A

A chemical property requires a chemical change in order to be observed.

Eg Reactivity and Ph

23
Q

What is a cation?

A

An ion that has lost electrons to gain a positive charge.

24
Q

What is an anion?

A

An ion that has gained electrons to gain a negative charge.

25
Q

What is the trend in the size of an atom on the periodic table?

A

The size of an atom increases down and to the left.

26
Q

What are isotopes?

A

Atoms with the same number of protons but different numbers of neutrons.

27
Q

What atomic particles determine an element’s physical and chemical properties?

A

Protons and neutrons

28
Q

What is a monatomic element? Give two examples.

A

An element that contains only one atom in its molecule.

Eg Iron and Carbon

29
Q

What is a diatomic element? Give two examples.

A

An element that contains two atoms in its molecule.

Eg Oxygen and Chlorine

30
Q

Does forming chemical bonds emit or require energy?

A

Emit energy.

31
Q

Does breaking chemical bonds emit or require energy?

A

Require energy.

32
Q

Describe the molecular structure of a metallic compound.

A

One type of ion surrounded by a sea of delocalised electrons.

33
Q

Describe the molecular structure of an ionic compound.

A

Two types of ions connecting to each other in a lattice.

34
Q

Describe the molecular structure of a covalent network compound.

A

A giant lattice of atoms.

35
Q

Describe the molecular structure of a covalent molecular compound.

A

Several atoms covalently bonded together.

36
Q

What is the difference between a small molecule and a big molecule?

A

Small molecules are limited in size, whereas big molecules are limitless in size.

37
Q

Describe the melting point and conductivity in solid and liquid state of metallic, ionic, covalent molecular and covalent network compounds.

A

Group Melting Point Solid Conductivity Liquid Conductivity
Metallic High High High
Ionic High Low High
Cov. Network High Low Low
Cov. Molecular Low Low Low

38
Q

A compound has a low melting point, low solid conductivity and low liquid conductivity.
What is most likely its molecular structure?

A

Covalent molecular.

39
Q

A compound has a high melting point, low solid conductivity and low liquid conductivity.
What is most likely its molecular structure?

A

Covalent network.

40
Q

A compound has a high melting point and low solid conductivity but high liquid conductivity.
What is most likely its molecular structure?

A

Ionic.

41
Q

A compound has a high melting point, high solid conductivity and high liquid conductivity.
What is most likely its molecular structure?

A

Metallic.

42
Q

What is the difference between the molecular and empirical formula of a molecule?

A

The molecular formula demonstrates how many atoms there are in one molecule, whereas the empirical formula demonstrates the ratio of atoms in one molecule.

43
Q

Out of metals, semi-metals and non-metals, which typically have a high melting or boiling point?

A

Metals and semi-metals.

44
Q

Out of metals, semi-metals and non-metals, which typically have low conductivity of heat and electricity?

A

Non-metals and semi-metals

45
Q

Out of metals, semi-metals and non-metals, which typically have a low melting or boiling point?

A

Non-metals

46
Q

Out of metals, semi-metals and non-metals, which typically have high conductivity of heat and electricity?

A

Metals.

47
Q

State two everyday examples of decomposition reactions.

A

Air bags
Sodium Azide -> Sodium + Nitrogen

Electrolysis
Aluminium Oxide -> Aluminium + Oxygen

48
Q

State two everyday examples of synthesis reactions.

A

Rust
Fe + O2 -> FeO

Pollution
N + O -> NO + NO2

49
Q

Explain the hardness and conductivity of metallic molecules.

A

Very hard, strong electrostatic attraction leads to strong bonds.

High conductivity, delocalised electrons allows for easy conductivity.

50
Q

Explain the hardness and conductivity of ionic molecules.

A

Hard, ions tightly bound by electrostatic forces.

Conductive when molten, mobile ions can easily conduct.

51
Q

Explain the hardness and conductivity of covalent molecular molecules.

A

Soft, weak intermolecular forces.

Low conductivity, molecules uncharged and electrons shared so they don’t easily flow.

52
Q

Explain the hardness and conductivity of covalent network molecules.

A

Hard but brittle, strong forces between atoms but distortion breaks covalent bonds.

Low conductivity, electrons localised in bonds leading to minimal electron flow.

Prelim Chemistry (3 decks)

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