Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Periodic Table Trends > Flashcards

Periodic Table Trends Flashcards

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

what is first ionisation energy

A

first ionisation energy as the removal of 1 mol of electrons from 1 mol of gaseous atoms

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

how is the periodic table arranged

A
  • by increasing atomic (proton) number
  • showing repeating trends in physical and chemical properties (periodicity)
  • in groups having similar chemical properties
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is metallic bonding

A

metallic bonding as strong electrostatic attraction between cations (positive ions) and delocalised electrons

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

what structure do all metals have

A

giant metallic lattice structure

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

examples of solid giant covalent lattices of carbon

A

diamond graphite and graphene

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

outer shell electron configuration of group 2 elements

A

outer shell electron configuration is s2

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

what ions are formed in redox group 2 reactions

A

loss of these electrons in redox reactions to form 2+ ions

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

a use of Ca(OH)2

A

in agriculture to neutralise acid

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

uses of Mg(OH)2 and CaCO3

A

antacids’ in treating indigestion.

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

nth ionisation energy equation

A

X(n-1)+(g) –> e- + Xn+(g)

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

where is the s-block

A

group 1 2 and H

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

where is the p-block

A

group 3 4 5 6 7 8

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

where is the d-block

A

transition metals

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

how would you describe solid giant covalent lattices of carbon (diamond, graphite and graphene) and silicon

A

as networks of atoms bonded by strong covalent bonds

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

the outer shell electron configuration of group 2

A

the outer shell electron configuration is s2

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

what ion do group two form

A

loss of these electrons in redox reactions to form 2+ ions

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

relative reactivities of the Group 2 elements Mg → Ba shown by their redox reactions with oxygen, water and dilute acids

A 
increases down group 
(reactions with water) 
Mg - VERY slowly
Ca - steadily
Sr - fairly quickly
Ba- rapidly
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

group 2 metal plus water

A

makes metal hydroxide and hydrogen

M + 2H2O –> M(OH)2 + H2

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

group 2 metal plus oxygen

A

forms solid white oxides

2M + O2 –> 2MO

20
Q

group 2 metal plus dilute acid

A

produces salt plus hydrogen
e.g. hydrochloric acid produces metal chloride and hydrogen
M + 2HCl –> MCl + H

21
Q

trend in reactivity in terms of ionisation energy down group 2

A

as you go down the group, ionisation energies decrease. this is due to increasing atomic radius and shielding effect.
when group 2 element react they lose electrons, forming cations. the easier it is to lose electrons ( lower the ionisation energies), the more reactive the element so reactivity increases.

22
Q

water and group 2 oxides

A

oxides of group 2 react readily with water to form metal hydroxides, which dissolve. the hydroxide ions OH-, make these solutions strongly alkaline.
(Mg is an exception - it only reacts slowly and the hydroxide isn’t very soluble)
the oxides form more alkaline solutions as you go down the group because the hydroxides get more soluble
e.g. CaO + H2O –> Ca2+ + 2OH-

23
Q

how do halogens exist

A

halogens exist as diatomic molecules

24
Q

explain the trend in the boiling points of Cl2, Br2 and I2, in terms of induced dipole–dipole interactions (London forces)

A

increase down the group because of the increasing strength of the London forces as the size and relative mass of atoms increases

25
Q

state the outer shell electron configuration of halogens

A

the outer shell electron configuration is S2P5

26
Q

what ions are formed in redox group 7 reactions

A

the gaining of one electron in many redox reactions to form 1– ions

27
Q

describe the trend in reactivity of the halogens Cl2, Br2 and I2

A

get less reactive down the group as the atomic radii increases so it is harder to attract an extra electron as the effective nuclear charge gets weaker.
halogens displace less reactive halide ions from solution

28
Q

what is disproportionation

A

oxidation and reduction of the same element in a reaction

29
Q

benefits of chlorine in water treatment

A

kills bacteria making water safe to drink
prevents reinfection
prevents algae growth, eliminating bad tastes and smells and removes discolouration

30
Q

risks of chlorine in water treatment

A

hazards of toxic chlorine gas

possible risks from formation of chlorinated hydrocarbons

31
Q

ethical considerations of using chlorine in water treatment

A

people should be able to choose what is in their water

32
Q

disproportionation reaction of water and chlorine

A

Cl2 + H2O –> HClO + HCl

33
Q

disproportionation reaction of chlorine with cold, dilute aqueous sodium hydroxide

A

Cl2 + 2NaOH –> NaCl + NaClO + H2O

34
Q

what is needed to form bleach

A

chlorine

cold, dilute aqueous sodium hydroxide

35
Q

what is the disproportionation reaction of chlorine with cold, dilute aqueous sodium hydroxide used for

A

to make bleach

36
Q

silver nitrate and ammonia test result for chloride

A

white precipitate, dissolves in dilute ammonia

37
Q

silver nitrate and ammonia test result for bromide

A

cream precipitate, dissolves in conc. ammonia

38
Q

silver nitrate and ammonia test result for iodide

A

yellow precipitate, in soluble in conc. ammonia

39
Q

ionic equation of halide plus silver nitrate

A

Ag+ + X- –> AgX (where X is Cl, Br or I)

40
Q

method for testing for halide ions

A

1) add dilute nitric acid (to remove ions that might interfere with the test)
2) add silver nitrate solution (AgNO3)
4) not colour of precipitate formed
5) if not clear add ammonia solution and check solubility

41
Q

how to detect carbonates

A

add a dilute acid and carbon dioxide will be released if carbonate present
CO3 2- + 2H+ –> CO2 + H2O

42
Q

how to test for carbon dioxide

A

lime water turns cloudy

43
Q

how to test for sulfates

A

add dilute HCl
add Barium Chloride solution BaCl2
if you get a white precipiate there was a sulphet present before
Ba2+ SO4 2- –> BaSO4

44
Q

how to test for ammonium compounds

A

add sodium hydroxide
warm mixture
hold a damp piece of red litmus paper over and see if it turns blue
if so ammonium ions present

45
Q

what order to test for substances in

A

1) carbonates
2) sulphates
3) halides

Chemistry (12 decks)

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