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Year 10 Chemistry > C4.1 > Flashcards

C4.1 Flashcards

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1
Q

elements in Group 1 of the periodic table

A

alkali metals

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2
Q

Define a catalyst

A

a substance that increases the rate of reaction, without being used up, by lowering the activation energy needed

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3
Q

Define crystalline

A

the structure of substances in the solid state that have particles arranged in a giant lattice

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4
Q

density

A

mass per unit volume,
measured in g/cm3 or kg/m3.
An object with high density is dense and feels heavy for its size

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5
Q

Define a displacement reaction

A

reaction in which a more reactive element displaces a less reactive element from it compounds

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6
Q

Noble gases are the name of elements in which group of the periodic table

A

Group 0, 8 or 18

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7
Q

Name of negative ions made from group 7 elements

A

halide ion

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8
Q

What are elements in Group 7 of the periodic table called?

A

halogens

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9
Q

What are monatomic elements

A

existing as single atoms, such as the noble gases

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10
Q

Define reactivity

A

the tendency of a substance to take part in chemical reactions

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11
Q

What are elements in the block of the periodic table between Groups 2 and 3 called

A

transition metals

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12
Q

describe trends in the physical properties of the Group 1 elements.

A

The alkali metals:

1 - are soft (they can be cut with a knife)

2 - going down group 1, the melting point decreases.

3 - Generally low densities. The first three (lithium, sodium and potassium float on water.

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13
Q

What happens when Group 1 elements react with water.

A

universal indicator turns solution blue or purple

Metal fizzes and dissolves (or catches fire)

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14
Q

What is the general balanced equation for the reactions of the Group 1 elements with water

A

2M(s) + 2H2O(l) → 2MOH(aq) + H2(g)

Alkaline metal + water → metal hydroxide + hydrogen

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15
Q

describe trends in the physical properties of the Group 7

A

The melting points and boiling points of the halogens increase going down group 7, and their colour gets darker.

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16
Q

use knowledge of electronic structures to explain in detail the trend in reactivity of the Group 1 elements.

A

A change like this, where an electron is lost, is an example of oxidation.

The ions formed have a stable electronic structure, like a noble gas from Group 0.

The reactivity of Group 1 elements increases as you go down the group because:

the atoms get larger as you go down the group
the outer electron gets further from the nucleus as you go down the group
the attraction between the nucleus and outer electron gets weaker as you go down the group - so the electron is more easily lost

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17
Q

Write the general balanced chemical equations for the reactions of Group 7 (IUPAC Group 17) elements with metals.

A

The halogens react with metals to produce salts

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18
Q

describe the trend in reactivity of the Group 7 (IUPAC Group 17) elements.

A

The halogens become less reactive going down group 7.

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19
Q

use knowledge of electronic structures to explain in detail the trend in reactivity of the Group 7 (IUPAC Group 17) elements.

A

Atoms of group 7 elements all have seven electrons in their outer shell.

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20
Q

What is the order of reactivity of the halogens to explain the outcome of a displacement reaction.

A

A more reactive halogen can displace a less reactive halogen from solutions of its salts.

F > Cl > Br >I

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21
Q

Write half equations for each reactant in a halogen displacement reaction between KI + NaCl

A

KI + NaCl ->

22
Q

identify which species have been oxidised and which have been reduced in the reactions between KI and NaCl

A

—

23
Q

the physical properties of a noble gas element

A

The noble gases all have low boiling points.

They are extremely unreactive and colourless.

This is because they have a full outer shell.

They cannot form bonds and therefore always exist as single atoms (monatomic).

24
Q

use knowledge of electronic structures to explain in detail the lack of reactivity of the noble gases.

A

—

25
Q

compare the physical properties of transition metals with those of Group 1 metals.

A

—

26
Q

describe how to distinguish transition compounds from each other and from Group 1 compounds

A

—

27
Q

describe some physical properties of transition metals.

A

—

28
Q

explain the use of transition metals as catalysts.

A

—

29
Q

describe how to distinguish transition compounds from each other and from Group 1 compounds.

A

—

30
Q

deduce the charge on a transition metal ion, given the formulae of its compounds.

A

—

31
Q

describe the products of a metal displacement reaction.

A

—

32
Q

use the relative strengths of the forces between atoms to explain the trend in boiling point of the noble gases.

A

—

33
Q

Describe group 1 element reactions with moist air

A

Group 1 elements are stored in oil to stop contact with air and water vapour.
Moist air reacts with alkaline metals to form the metal oxide. This tarnishes the surface of the metal.

34
Q

What would you observe when lithium reacts with water?

A

Fizzes steadily, and slowly becomes smaller until it has all reacted

35
Q

Describe what you would observe when sodium reacts with water.

A

Melts to form a ball, fizzes rapidly, and quickly becomes smaller until it disappears

36
Q

What would you observe when potassium reacts with water?

A

Quickly melts to form a ball, burns violently with sparks and a lilac flame, and reacts rapidly, often with a small explosion

37
Q

Predict what is seen when rubidium is added to water.

A

Rubidium should melt very quickly. It should burn very violently, and react almost instantly with an explosion.

38
Q

What are the physical properties of group 7 elements?

A

The group 7 elements exist as diatomic molecules. Their chemical formulae are F2, Cl2, Br2 and I2.

Group 7 elements have low boiling points.

39
Q

What is the standard state of chlorine?

A

Cl2 = Yellow-green Gas

40
Q

What is the standard state of bromine?

A

Br2 = Deep-red Liquid

41
Q

What is the standard state of iodine?

A

I2 = Grey Solid that easily sublimes into a Purple gas

42
Q

What is a hazard of chlorine gas in the lab?

A

Toxic if inhaled. Make sure the lab is well ventilated and avoid inhaling.

43
Q

What is a hazard of bromine in the lab?

A

Bromine vapour is toxic. Solution irritates the skin. Make sure the lab is well ventilated and avoid inhaling the vapour. Wear gloves

44
Q

What is a hazard of iodine in a lab?

A

Iodine is harmful to the skin. Wear gloves. Avoid contact with clothing.

45
Q

What do you observe when potassium chloride with chlorine

A

No change

46
Q

What do you observe when potassium bromide reacts with chlorine

A

Solution darkens as bromine is produced

47
Q

What do you observe when potassium iodide is reacted with bromine?

A

Solution darkens as iodine is produced

48
Q

Describe what you would observe when potassium bromide reacts with iodine.

A

No change

49
Q

Describe the reactivity of group 1 elements

A

The Group 1 elements have similar properties because of the electronic structure of their atoms - they all have one electron in their outer shell.

In a reaction, an atom of a Group 1 element will form an ion with a single positive charge.

49
Q

Describe the trend in reactivity of group 1 elements.

A

The reactivity of Group 1 elements increases as you go down the group because:

the atoms get larger as you go down the group
the outer electron gets further from the nucleus as you go down the group
the attraction between the nucleus and outer electron gets weaker as you go down the group - so the electron is more easily lost

Year 10 Chemistry (7 decks)

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