Module 3: Periodic Table and Energy Flashcards Preview

OCR A Level Chemsitry > Module 3: Periodic Table and Energy > Flashcards

Flashcards in Module 3: Periodic Table and Energy Deck (71):
1

How were elements grouped in the 1800s?

Atomic mass

2

How was the modern priodic table created?

Mendeleev

3

How does the periodic table arrange elements?

By proton number

4

Where are the P, S, D and F blocks in the periodic table?

can be used to work out electron configurations

5

What is ionisaiton?

The removal of one or more electrons

6

Name factors affecting ioniation energy.

RNS

7

How does ionisation energy change down a gorup?

Decreases

8

How does ionisation energy change across a period?

Increases

9

Why is there a drop in ionisation energy between groups 2-3?

Added to new shells

10

Why is there a drop in ionisation energy between groups 5-6?

P orbital repulsion

11

Give one key peice of evidence for electron shell structue.

Sucessive ionisation energies

12

What are the structures of graphite and graphene?

Covelant lattices

13

Explain the properties of diamond in terms of bonding and structure.

Hardest known substance

14

Explain the properties of graphite in terms of bonding and structure.

Slippery

15

What is the difference between graphene and graphite?

Layers

16

Explain the properties of metals in terms of bonding and strcture.

Metallic bonding.

17

Explain the properties of simple molecular compounds in terms of bonding and structure.

Weak IM bonds

18

How and why do melting and boiling points change across a period?

Due to bond strength

19

Give the relative melting and boiling points of:
1) Ionic compounds
2) Simple molecular substances
3) Giant covelant lattices and
4) Metallic compounds

High low high high

20

Give the states at RTPof:
1) Ionic compounds
2) Simple molecular substances
3) Giant covelant lattices and
4) Metallic compounds

s, varying, s, s

21

Which of the following conduct electricity?
1) Ionic compounds
2) Simple molecular substances
3) Giant covelant lattices and
4) Metallic compounds

For varying states (both)

22

Which of the following are soluble in water?
1) Ionic compounds
2) Simple molecular substances
3) Giant covelant lattices and
4) Metallic compounds

Y, deps, no

23

What ions do group 2 elements form?

2+

24

How does reactivity change down group 2?

Increases

25

Name three reactions of group 2 elements.

Hydroxides ect

26

Name the trends in the alkalinity of group 2 alkalais.

Increases

27

Name uses of group 2 compounds.

give eq in

28

Give the colours and standard states of group 7 elements.

are diatomic;

29

Explain the trend in reactivity down group 7.

Less reactive ox agents

30

In halogen displacement reactions, each halide ion produces a different colour. Name and explain these colours.

Rel ox strengths

31

Give the ionic equation for the displacement if bromine by chlorine, reacting with KCl.

eq

32

Name the halide test? Give an ionic equation.

Ionic eq

33

Name disproportinaton reactions, giving a use of chlorine.

two

34

Outline the benefits, risks and ethical implications of utilising chlorine.

+/-...

35

Name the carbonate test.

IIncluude reaction

36

Name the sulphate test.

Equation

37

ADD "TEST FOR HALIDES WITH AGNO3" TO NAME HALIDE TEST CARD

...

38

Name the test for ammonium compounds.

Eq, = alkalai

39

In what order should ion tess be done and why?

False +ives

40

What is ΔH^⊖?

standard cond's

41

What are the corresponding values of ΔH for exothermic and endothermic reactions? Name examokes of these reactions.

Give eqs

42

List the features of an enthalpy profile diagram.

axo, endo

43

What are the conditions for enthalpy changes?

st

44

Define:
1) ΔHr^⊖
2)ΔHf^⊖
3)ΔHc^⊖
4) ΔHneut^⊖

define

45

What are the respective values of ΔH for making and breaking bonds?

h

46

Why is energy needed to break bonds?

overcome attractive IM f's

47

Name flaws in the methods for calculating average bond enthalpies.

list

48

Design an expreiment to calcluate enthalpy change of combustion of a substance.

MAP

49

How can enthalpy changes be calculated from a calorimetry experiment?

-q/n

50

What is Hess's Law, and when is it useful?

Indep

51

Compare and contrast methods for working out the enthaply changes of formation and combustion via Hess's Law.

compare triangles, be ware of molar ratios/ balance eqs

52

Give a formula for the enthalpy change of reaction.

formula

53

Name two conditions for the sucessful colliosions of particles, define activation energy.

ENTHALPY PROFILE DIAGRAM "List the features of an enthalpy profile d" card

54

What do the axies of a Boltzman distribution look like? Liist the features of such a distribution.

Thr origin, x ax axymptote

55

What effect would increasing the temparature have on the look of the Boltzman distribution of a reaction?

shifts, Ea same - more p's above threshold

56

Name the effects of increasing:
1) Concentration
2) Pressure, and
3) Use of catalysts
On a reaction mixture.

name - cataly b man distrib

57

What is a catalyst, in the context of a dymnamic equillibrium?

name

58

What evidence is there that catalysts work?

Enthalpy profiles and b man d's

59

Name and explain two types of catalysts.

Hetero , homeo

60

Name advantages of catalysts.

name, for both boxes

61

Give an equation to calculate rate of reacion.

stuff/time

62

Name two methods of investigating rates of reaction.

mass change, gas volume produced

63

How can the rate of reaction be calculated from a graph?

For both boxes

64

What are the conditions for a dynamic equillibrium?

Cloasedsy, exp what is

65

What is Le Chatlier's Principle?

give

66

Explain a change in:
1) Concentration
2) Pressure and
3) Temparature
Via Le Chatlier's Principle.

Exp

67

How do catalysts affect the position of equillibrium?

They don't

68

Name:
1) The general equation
2) The specific equation and
3) The conditions
For the formation of ethene.

From steam

69

How cant the equillibrium constant be calculated, and what does it mean?

p/ re's - means if huge, then re favious prods, pos of eq
no units
for both boxes

70

Design a practical, which investigates the equillibrium position of a given reaction with changing temperature.

NO2 exp

71

Design a practical, which investigates the equillibrium position of a given reaction with changing pressure.

Fe3+ exp