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Chemistry year 9 > C1 + C2 > Flashcards

C1 + C2 Flashcards

1
Q

What is an atom?

A

The smallest particle of an element that can exist

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2
Q

Why do some elements form ions?

A

Elements form ions to

get a full outer shell, which is more stable

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3
Q

What charge would a sodium ion have?

A

+1

Sodium is in Group 1.

It has one electron in its outer shell.

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4
Q

What is an isotope?

A

An isotope is

an atom that has more neutrons than usual (but the same number of protons).

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5
Q

What is an element?

A

A substance that contains only one sort of atom

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6
Q

What is a compound?

List the elements in these compounds:

  1. CaSO4
  2. Magnesium nitrate Mg(NO3)2
A

A substance that is made of two or more different types of atoms that are chemically bonded together.

  1. calcium,sulfur, oxygen
  2. magnesium, nitrogen, oxygen
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7
Q

What is a solvent?

A

The liquid that does the dissolving.

e. g. the water in sea water

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8
Q

What is a solution?

A

Liquid with solid disolved in.

e. g. sea water (liquid and solid together)

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9
Q

What is a solute?

A

Solid that gets dissolved.

e. g. the salt in the sea water

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10
Q

What is soluble?

A

can dissolve in liquid

e. g. salt is soluble in water

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11
Q

What is insoluble?

A

Can not dissolve.

e. g. sand is insoluble in water

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12
Q

Filtration

What is this separation technique used for?

A

Filtration separates insoluble solids from mixtures.

e.g. sand can be separated from salt using filtration

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13
Q

What is this separation technique used for?

Distillation

A

Distillation is separating mixtures of liquids with different boiling points.

e.g. pure water can be distilled from sea water

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14
Q

Evaporation

What is this separation technique used for?

A

Evaporation is used to remove solvents from solutions.

e.g. a salt can be separated from a solution by heating it until the solvent (liquid) evaporates.

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15
Q

Chromatography

What is this separation technique used for?

A

Chromatography is used for separating dyes from mixtures.

e.g. different dyes in food colourings

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16
Q

What was the plum-pudding model of an atom?

A

A ‘blob’ of positive charge with negative charged electrons arranged at random throughout.

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17
Q

What did Rutherford discover and how did he observe it?

A

He discovered the nucleus by firing alpha particles at a thin gold sheet of foil and observing their interaction. He saw roughly 1/7000 particles were reflected back, indicating a solid nucleus at the core.

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18
Q

Explain how Mendeleev arranged the elements in the Periodic Table. Why did he leave gaps?

A

He organised the Periodic Table

in order of increasing atomic mass.

He left gaps for undiscovered elements.

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19
Q

Complete the following word equations:

  1. Potassium chloride + fluorine
  2. Sodium fluoride + iodine
  3. Magnesium iodide + bromine
A
  1. Potassium fluoride + chlorine

2. NO REACTION

  1. Magnesium bromide + iodine
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20
Q

Which are the properties that you would expect magnesium to have?

Sonorous, low boiling point, hard,

dull, brittle, insulator, ductile, conductor

high melting point

A

Sonorous

ductile

conductor

high melting point

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21
Q

Balance the following equations:

H2 + Cl2 → HCL

Zn + O2 → ZnO

Cl2 + Al → AlCl3

Fe2O3 + Al → Fe + Al2O3

A

H2 + Cl2 → 2 HCL

2 Zn + O2 → 2 ZNO

3 Cl2 + 2 Al → 2 AlCl3

Fe2O3 + 2 Al → 2 Fe + Al2O3

22
Q

What is the mass and the charge?

23
Q

What are the number of protons, electrons, neurons and Electronic structure?

24
Q

Complete the equations:

25
Q

Label the diagram, describe the structure, name the element shown

26
Q

What are mixtures?

A

Two or more elements or compounds which are NOT CHEMICALLY COMBINED

27
Q

How can mixtures be separated?

A

mixtures can be separated by:

  1. filtration
  2. evaporation (crystallisation)
  3. distillation
  4. chromatography
28
Q

How is an element different to a compound?

A

Elements contain just one type of atom, compounds contain atoms of at least two different elements which have been chemically combined

29
Q

What does the formula CaCO3 tell you about the compound calcium carbonate?

A

It contains:

1 Calcium atom

1 carbon atom

3 Oxygen atoms

30
Q

What process can be used to extract pure water from salt water?

A

Simple distillation

31
Q

What do atoms contain?

A

Subatomic particles called:

Protons

Neurons

Electrons

32
Q

What is the charge or Protons?

What is the relative mass of protons?

A

Protons

Charge: +1

Relative mass: 1

33
Q

What is the charge of Neutrons?

What is the relative mass of Neutrons?

A

Neutrons

Charge: no charge

Relative mass: 1

34
Q

What is the charge of electrons?

A

Electrons

Charge: -1

Relative mass: very small

35
Q

What is the top number on a symbol?

A

The Mass number (number of protons + neutrons)

36
Q

What is the bottom number on a symbol?

A

The atomic number (number of electrons)

37
Q

How do you calculate the number of neutrons?

A

Top number - Bottom number = number of neutrons

38
Q

What is the electronic structure of an atom?

A

Shows how the electrons are arranged around the nucleus in shells (energy levels).

first shell = max 2 electrons

next two shells= max 8 electrons

39
Q

An atom of potassiu has an atomic number of 19 and a mass number of 39. State the number of protons, electrons and neutrons of this atom.

A

19 Protons

19 Electrons

20 Neutrons

40
Q

An ion of potassium -39 has a +1 charge. State the number of protons, neutrons and electrons in the ion.

A

19 protons

18 electrons

20 neutrons

41
Q

How are the elements in the periodic table organised?

A

Elements that have the same number of electrons in their outer shell have similar properties.

They are in the same group.

e.g. Group 1 elements all have one electron in their outer shell

42
Q

What group are noble gases in?

Why are the very unreactive?

A

Group 0

They are unreactive because their outer shell of electrons is full so they don’t need to react with other elements.

43
Q

What are group one elements called? What are their properties?

A

Alkali metals

  • They have one electron in their outer shell.
  • they have low melting and boiling points
  • they are very reactive with oxygen and water
  • they have low density
  • they react with non-metals to form ionic compounds
44
Q

How do group one elements change going down the group?

A
  • boiling and melting points decrease
  • they become more reactive as the outer electron is lost more easily
45
Q

What do group 1 metals from with oxygen?

eg. sodium + oxygen = ?

A

They form metal oxides.

eg. sodium + Oxygen= sodium oxide

46
Q

What happens when lithium, sodium and potassium are put in water? Why?

A

They float on top of it because they are less dense than water.

47
Q

How do alkali metals react with water?

eg,

potassium + water = ?

A

They form a metal hydroxide and hydrogen gas is given off.

eg.

potassium + water = potassium hydroxide + hydrogen

48
Q

What are the group 7 elements called? What are their properties?

A

They are non-metals known as halogens.

  • they have 7 electrons in their outer shell
  • they react with metals to produce salts
  • The reactivity decreases down the group as it becomes less easy to gain an electron
  • A more reactive halogen will displace a less reactive halogen
49
Q

What are the diplacement reactions?

Chlorine + Potassium bromide = ?

chlorine + potassium iodide =?

bromine + potassium iodide=?

A

Chlorine will displace bromine from potassium bromide

chlorine + potassium bromide = potassium chloride + bromine

chlorine + potassium iodide = potassium chloride + iodine

bromine + potassium iodide= potassium bromide + iodine

50
Q

Why are group 0 elements unreactive?

A

They have a full outer shell which is a stable arrangement.

51
Q

Why are alkali metals stored in oil?

A

Because they are highly reactive they are stored in oil to

To stop them from reacting with oxygen or water (moisture) in the air

Chemistry year 9 (2 decks)

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