Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

AS Chemistry Unit 1 + 2 > Unit 1.6 - Periodic Table > Flashcards

Unit 1.6 - Periodic Table Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

1) What does the group number tell you?
2) What does the period number tell you?
3) What block are the transition metals in?

A

1) Number of electrons in outer shell.
2) Number of quantum shells containing electrons.
3) D block

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

When was the periodic table produced?

A

Mendeleev in 1869.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is periodicity?

A

Name given to any pattern in physical or chemical properties that appears across a period.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

State the order of bond strength.

A

Giant covalent > metals > simple molecular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Why does metallic bonding have a higher boiling point than melting point?

A

Liquid state but atoms are separated to distances forming the vapour and this involves breaking of metallic bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

2nd period - State the type of structure in:

1) Li and Be
2) B and C
3) N, O and F
4) Ne

A

1) Giant metallic
2) Giant covalent
3) Simple covalent
4) Simple atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

3rd period - State the type of structure in:

1) Na, Mg and Al
2) Si
3) P, S and Cl
4) Ar

A

1) Giant metallic
2) Giant covalent
3) Simple covalent
4) Simple atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

1) What is atomic radius?

2) What method is used to determine atomic radii?

A

1) Measure of size of atoms in crystals and molecules.

2) X-ray diffraction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

1) What is the trend in atomic radii across a period?

2) Explain why.

A

1) Atomic radii decrease across period.

2) Increase in nuclear charge, no increase in electron shielding and increase in effective nuclear charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

1) What is the trend in atomic radii down any group?

2) Explain why.

A

1) Increases down any group.

2) Number of electron shells increases.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

1) What is the trend in 1st ionisation energy across a period?
2) Explain why.

A

1) Increases across period.
2) Increase in nuclear charge in same energy level, little extra shielding and greater attraction between nucleus and outer electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

1) What is the trend in 1st ionisation energy down a group?

2) Explain why.

A

1) Decreases down group.

2) Increase in nuclear charge, increase in electron shielding and decrease in effective nuclear charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Electronegativity

A

Ability of an atom to attract a shared pair of electrons towards itself in a covalent bond.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

1) What is the trend in electronegativity across a period?

2) Explain why.

A

1) Increases across period.

2) Increase in nuclear charge, no increase in electron shielding and increase in effective nuclear charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

1) What is the trend in electronegativity down a group?

2) Explain why.

A

1) Decreases down each group.

2) Increase in nuclear charge, increase in electron shielding and decrease in effective nuclear charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

1) What happens to an element when oxidation number increases?
2) What happens to an element when oxidation number decreases?

A

1) Lost electrons - Oxidised

2) Gained electrons - Reduced

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Describe observations when:

1) Lithium reacts with water
2) Sodium reacts with water
3) Potassium reacts with water

A

1) Floats, moves slowly, effervescence and fizzing sound.
2) Faster, effervescence and orange spark.
3) More reactive, lilac burning flame and vigorous effervescence.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

1) State and explain the general trend in reactivity of group 1 and 2 down the group.
2) Why do group 1 melt with cold water but group 2 don’t?

A

1) Increases down group - nuclear charge increases, increase in electron shielding and decrease in effective nuclear charge as becomes easier to loose valence shell electron.
2) Group 1 - more exothermic and float
Group 2 - Higher melting point and don’t float.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

State the general equation for metals when:

1) Group 1 reacts with water
2) Group 2 reacts with water

A

1) 2 M + 2 H2O > 2 MOH + H2

2) M + H2O > M(OH)2 + H2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Explain why group 1 elements float on the water surface during a reaction.

A

Group 1 are less dense than water, group 2 have a higher density.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

1) What is the general equation when metal reacts with water?
2) What is the general equation when metal reacts with acid?

A

1) Metal + Water > Salt + Hydrogen
2) Metal + Acid > Salt + Water

Metals are good reducing agents.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Mg + 2HCl > MgCl2 + H2

What would happen if dilute sulphuric acid was used?

A

Sulphate salt would be produced.

23
Q

1) What solution is formed when oxides react with water (group 2)?
2) State an example.
3) State an example when elements react with oxygen.

A

1) Alkaline solutions
2) CaO + H2O > Ca(OH)2
3) 2 Mg + O2 > 2 MgO

24
Q

1) What is the equation when magnesium oxide reacts with dilute acids?
2) What are the oxides acting as?

A

1) MgO + 2 H+ > Mg2+ +H2O

2) Acting as bases.

25
Q

1) What is the general equation when group 1 metals react with oxygen?
2) What is the general equation when group 1 metals react with water?

A

1) 4 M + O2 > 2 M2O

2) 2 M + 2 H20 > 2 MOH + H2

26
Q

What compound and precipitate is formed when Mg2+ reacts with:

1) Na2SO4
2) Na2CO3
3) NaOH

A

1) MgSO4 (aq) -no ppt
2) MgCO3 (s) - white ppt
3) Mg(OH)2 (s) - white ppt

27
Q

What compound and precipitate is formed when Ca2+ reacts with:

1) Na2SO4
2) Na2CO3
3) NaOH

A

1) CaSO4 (aq) - slight ppt, sparingly soluble
2) CaCO3 (s) - white ppt
3) Ca(OH)2 (aq) - sparingly soluble, slight ppt

28
Q

What compound and precipitate is formed when Ba2+ (test for sulphate ions) reacts with:

1) Na2SO4
2) Na2CO3
3) NaOH

A

1) BaSO4 (s) - white ppt
2) BaCO3 (s) - white ppt
3) Ba(OH)2 (aq) - no ppt

29
Q

What does aq and s mean?

A

aq - soluble

s - insoluble

30
Q

1) Are group 2 carbonates soluble or insoluble?
2) What is trend in group 2 sulphates as you go down the group?
3) What is trend in group 2 hydroxides as you go up the group?

A

1) Carbonates all insoluble.
2) Sulphates less soluble down the group.
3) Hydroxides less soluble up the group.

31
Q

Explain how flame tests can be used in qualitative analysis.

A

All common elements in group 1 & 2 (except Mg) show characteristic flame colours that can be used to identify them.

32
Q

State the flame colour of:

1) Lithium
2) Sodium
3) Potassium
4) Magnesium
5) Calcium
6) Strontium
7) Barium
8) Copper

A

1) Red
2) Yellow/Orange
3) Lilac
4) Colourless
5) Brick red
6) Crimson red
7) Apple green
8) Green

33
Q

1) State an example when group 2 carbonates undergo thermal decomposition.
2) What happens to carbonates as you go down the group?

A

1) CuCO3 (s) [blue/green] > CuO (s) [black] + CO2 (g)

2) Carbonates become more stable to heat as you go down the group.

34
Q

1) State the general equation for when group 2 hydroxides undergo thermal decomposition.
2) What happens to hydroxides as you go down the group.

A

1) X(OH)2 (s) > XO (s) + H2O (g)

2) Hydroxides become more stable to heat as you go down the group.

35
Q

State at room temperature:

1) Chlorine and fluorine.
2) Bromine.
3) Iodine.

A

1) Gas
2) Liquid
3) Solid

36
Q

What happens to the volatility of group 7 as you go down the group?

A

Less volatile, boiling points decrease due to higher Mr (size of atom increases), more electrons, stronger Van Der Waals forces between molecules.

37
Q

Describe the reactivity of group 7 as you go down the group.

A

Less reactive as they need to gain an electron, greater electron shielding and decrease in effective nuclear charge.

38
Q

State whether a reaction occurs:

1) Cl2 + KCl
2) Cl2 + KBr
3) Cl2 + KI

A

1) -
2) KCl + Br2
3) KCl + I2

39
Q

State whether a reaction occurs:

1) Br2 + KCl
2) Br2 + KBr
3) Br2 + KI

A

1) x
2) -
3) KBr + I2

40
Q

State whether a reaction occurs:

1) I2 + KCl
2) I2 + KBr
3) I2 + Ki

A

1) x
2) x
3) -

41
Q

What is observed when group 7 elements react with metals?

A

Colourless crystalline salt, reactivity decreases down group 7 vice versa for group 1.

42
Q

Describe how halide ions are identified. What is the importance of dilute nitric acid?

A

Silver nitrate test - dilute nitric acid added to solution, silver nitrate added. Dilute nitric acid prevents precipitation of any other salts.

43
Q

How do you test the solubility of a precipitate?

A

Dilute and concentrated ammonia solution.

44
Q

State observation when NaCl is added to:

1) AgNO3
2) NH3

A

1) White ppt

2) Dissolves in aqueous/clear solution

45
Q

State observation when KBr is added to:

1) AgNO3
2) NH3

A

1) Cream ppt

2) Dissolves in concentrated ammonia - cloudy in dilute so doesn’t dissolve.

46
Q

State observation when KI is added to:

1) AgNO3
2) NH3

A

1) Yellow ppt

2) Insoluble : doesn’t dissolve

47
Q

State the advantages of chlorination and what it helps to prevent.

A

Kills microbes and bacteria, prevents outbreak fo diseases such as typhoid, cholera and dysntery.

48
Q

What are the disadvantages of chlorination?

A

Highly toxic, react with organic compounds found in water supply (tirhalomethanes) to form chlorinated hydrocarbons which cab cause liver and kidney cancer.

49
Q

State an advantage of fluoridation.

A

Reduces tooth decay by preventing cavities.

50
Q

What are the disadvantages of fluoridation?

A

Cosmetic purposes, causes fluorosis (leads to tooth discolouration), forced mass medication as already in toothpaste and mouthwash.

51
Q

State whether the following are soluble or insoluble:

1) Group 1 & ammonium compounds
2) Nitrates
3) Carbonates
4) Halides
5) Sulphates

A

1) Soluble
2) Soluble
3) Insoluble
4) Soluble except lead and silver halide
5) Soluble except lead and barium sulphate

52
Q

How can we separate a soluble salt?

A

Crystallisation: heating & evaporating solution to half its original volume, leaving remaining solution to evaporate slowly. Crystallise and be filtered.

53
Q

How can we separate an insoluble compound?

A

Appear as precipitation, separated by filtration.

54
Q

Volatility

A

How readily a substance vaporises.

AS Chemistry Unit 1 + 2 (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions