Brainscape's Knowledge GenomeTM

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


See full index

Science 2024 > C2 > Flashcards

C2 Flashcards

You may prefer our related Brainscape-certified flashcards:
Biology 101 flashcards
1
Q

Characteristics of period 1

A

Contains hydrogen and helium that are both gases
Electrons in these elements fill 1s orbital
Helium only hasn2 electrons and is unreactive
As hydrogen readily loses/gains electron it can behave as both group1/7 element
Hydrogen can form with most elements

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

Characteristics of period 2

A

Outer electrons in these elements dill the 2s and 2p orbitals
Nitrogen, oxygen and fluorine can all form diatonic molecules, neon is a noble gases and carbon is a giant molecular structure

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

Characteristics for period 3

A

Contains 8 elements, the outer electrons in these elements fill the 3s and 3p orbitals

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

Characteristics of period 4

A

Contains 18 elements. The first row of the transition elements is in this period. The outer electrons of these elements fill the 4s,4p and 3d orbitals

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

What is an element block

A

They are named for the orbital that rhe highest energy electrons are in that set of elements. Group 1 and 2 of the periodic table are in s block. Group 3 to 7 and Group 0 make up b block. This block contains all non metals except hydrogen and helium. The transition metal are in the d block

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

Examples of physical properties of elements

A

Atomic radius, ionic radius, electronegativity, first ionisation energy and reasons for trends, electron affinity, type of bonding in the element,melting point and boiling point, thermal and electrical conductivity, malleability and ductility

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

How do you measure the radius of an atom

A

Measure the distance between the nuclei of two touching atoms and divide by two

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

What happens to the atomic radius when going from the period left to right

A

Decreases but across the group more protons and electrons are added which means the electrons increase the nuclear charge but electrons are added to the same s and p sub shells so the size does not increase. The increased nuclear charge attracts the extra electrons and pulls them closer to the nucleus which leads to a decrease in atomic radius

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

What happens to the atomic radii as you go down

A

Increases as due to the extra electrons are added to additional shells this leads to the radius increasing. Although nuclear charge increases, the number of inner shells increase and so the nuclear charge is shielded more which means the atomic radius increases

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

How does atomic radii react with transition metals

A

Aortic radii gets slightly smaller as you go across the start of the transition metals but then the atomic radii stays very similar this is because the additional nuclear charge is balanced by extra shielding by the 3d electrons of the outer 4b sub shell

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

Why does ionic radius have a similar pattern to atomic radius

A

Because the extra electrons are added to extra shells as you go down the group therefore giving a larger size

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

Cations meaning

A

Ions with a positive charge

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

Isoelectronic meaning

A

Having the same number of electrons

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

What happens to cations when going across a period

A

Cations have a smaller radius than corresponding atom. As you go across a period ghe cations all have the same electronic structure but are electronic which means the nuclear charge inc4eaee across the period which pulls the electrons more strongly to the centre of ion so the cations decrease as you go a cross a period

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

Anions

A

Ions with a negative charge

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

What happens to ionic radius of anions when you go a cross a period

A

Have a larger radius than atom as there is more repulsion between the extra electrons. Anions are all isoelectronic and number of protons increase as go across period but number of shells and electrons stay the same, so ionic radius of Anions decrease as going across period

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

Electronegativity

A

Measure of tendency of an atom to attract a bonding pair of electrons

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

What happens to electronegativity across a period

A

Increases and the bonding pair of electrons will be shielded by the same number of electrons however the number of protons will increase so group 7 will be more electronegative than group 1 element

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

What happens to electronegativity across a group

A

Decreases which means fluorine is the most electronegative element
Group 0 gases do not form bonds and do not have electronegativity that can be reliably determined

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

What does electronegativity depend on

A

The number of protons in the nucleus, the distance from the nucleus of the bonding pair of electrons and how much shielding their is from the inner electrons

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

What happens to electronegativity as you go down the group

A

More shielding from inner electrons and the bonding pair of electrons are further from nucleus. This adds up to less pull on the bonding pair from the positive charge of the nucleus and so electronegativity decreases

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

First ionisation energy

A

The energy needed for one mole of electrons to be removed from one mole of gaseous atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Periodicty

A

The repeating pattern seen by the elements in the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

How is periodicity seen in relation to first ionisation energy

A

There is an overall trend of first ionisation energy increasing across the period

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Why is it harder to remove an electron as you go across a period

A

Because the number of protons increase across the period so the positive charge on rhe nucleus increases which means the force of attraction pulling on the outer electron increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Electron affinity

A

The change in energy when one mole of gaseous atoms gains one mole of electrons to form a mole of negative ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What are the elements that are included in the first electron affinity

A

Fluorine, chlorine bromine and iodine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What are first electron affinities

A

When a -1 ion is formed and are negative
The negative sign shows that the energy has been released plus the amount of energy released usually decreases as u go down group 7 but fluorine is an exception.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is the first electron affinity for fluorine

A

-328

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is the first electron affinity for chlorine

A

-349

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What is the first electron affinity for bromine

A

-324

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What is the first electron affinity fot iodine

A

-295

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

What does electron affinity indicate for group 7

A

How strong the attraction is between the nucleus of an atom and the incoming electron if this attraction is strong more energy is released

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What has an effect on electron affinity

A

Number of protons/nuclear charge is distance a nucleus and shielding
Aa you go down the group nuclear charge increases and the furthere the outer shell is from the positive pull of the nucleus attractions become weaker which means that less energy is released when the ion is formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Why does fluorine not follow electron affinity pattern

A

Because amall atom and when it becomes fluoride this new electron is added to a region that is already full of electrons and so there is repulsion from these

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

How is group 6 similiar to group 7s electron affinity

A

Follows similar pattern but oxygen does not follow this pattern
Group 6 have overall lower affinities than group 7 because they have one less proton but the same amount of shielding
Group 6 will also have a second electron affinity where the negative ion gains a asecond electron forming a charge of -2
The two negative charges will repel so this change in ergy will be positive and will be needed to force an electron into the negative ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What can be used to predict the type of bonding in a compound

A

Electronegativity

38
Q

Can you directly measure electronegativity of an element

A

No but the chemist Linus Pauling produced a scale that gives a relative value for the elements and allows you to predict how ionic a covalent bond will be

39
Q

Qhat does it mean if the electronegativities of the elements forming bonds are low

A

The covalent bond will be less polar than the difference between the electronegativities is high. As the difference increases, the covalent bond will become more polar and if the difference is very large then the bond becomes ionic

40
Q

How do ionic bonds show polarity

A

Whether ion is highly charged
Whether the cation is relatively small as this will draw electrons to it
Whether the anion is relatively large as it will have an electron cloud that is easily distorted which means that some of the negative charge is shared with the cation which gives the ionic bond some covalent characteristics

41
Q

What do melting and boiling points depend on

A

The strength of the forces between the atoms in an element

42
Q

What is the melting ang boiling point going down group 1 and 7

A

Decreases which means the forces of attraction are weaker
And Increases which means stronger

43
Q

How will u get a high melting and boiling point

A

The stronget the forces of atoms as when an element melts energy is used to overcome some of the attractive forces holding the atoms and molecules of the element together
When an element boils most of the rest of the attractive forces are broken

44
Q

What happens when you go across period 1 to 3

A

Metals have increasing nuclear charge because they have increasing number of protons and increasing number of delocalised electrons and so have a stronger metallic bonding which means the melting and boiling points increase across the period

45
Q

Why does carbon have a high melting and boiling point

A

Strong covalent bonds that need energy to break.however non metals between group5-7 have small separate molecules so have low melting point and are only weak van der walls forces that need to be overcome

46
Q

Why does sulfur have a higher melting and boiling pointthan the rest of non metals in period 3

A

Due to the different sizing of molecules and the strength of the van der waal force increases as the size of the molecul3s increase
Therefore because sulfur has the biggest molecule it has the strongest van der waal force so highest melting and boiling point

47
Q

What bond has the best for electrical conductivity

A

Copper and metallic bonding which allows electrical conductivity through a solid or liquid metal

48
Q

What do delocalised electrons do in electrical conductivity and why are they good

A

Carry the electrical charge and absorb heat energy which gives them kinetic energy. This energy is transferred through the metal by these electrons

49
Q

Are metals good thermal conductors malleable and ductile

A

Yes aluminium is a very good example
The atoms in the layers are able to roll over each other and they can move into new positions without breaking metallic bonds

50
Q

Chemical properties of element example

A

Elements reactions to oxygen,water,dilute hydrochloric acid and dilute sulfuric acid
Position on reactivity table,
Oxidation and reduction,
Variable oxidation states of transitional metal ions
Displacement reactions of metals/halogens

51
Q

How does group 1 elementa react with oxygen

A

Lithium and sodium make rapid burns with red flame
Metal oxide is produced that forms a alkaline solution when dissolved in water
Very vigorous,burns with orange flags
Metal oxide produced that form basic solution when dissolved in water

52
Q

How does group 2 elements react with oxygen

A

Beryllium and magnesium
Needs hat to reach as to do with group 1 elements and very vigorous reactions

53
Q

How does group 3 elements aluminium react with oxygen

A

Vigorous at first rapidly forms a water insoluble coating and this layer prevents the aluminium below from corroding which makes aluminium a useful material

54
Q

How does group 4 carbon and silicon react with oxygen

A

Forms slightly acidic oxides that shows reaction with heat but no reaction

55
Q

How does group 5 elements nitrogen and phosphorus react with oxygen

A

Forms a range of oxides eith different oxidation states a high temperature is needed for these reactions to take place
Burns vigorously with white flame

56
Q

How does group 6 elements oxygen and sulfur react with oxygen

A

In ozone layer
Two oxides form
Burns slowly with blue flame

57
Q

How does group 7 elements e.g halogens react with oxygen

A

Unstable oxides form

58
Q

How does group 0 elements neon and argon react with oxygen

A

No reaction

59
Q

Alkaline solution meaning

A

A solution with a pH above 7

60
Q

Oxidisation meaning

A

Loss of atoms/electrons

61
Q

Allotropes meaning

A

Two or more different physical forms that an element can exist in

62
Q

Amphoteric meaning

A

Substance that can act as both an acid and a base

63
Q

When group 1 reacts with water what do they produce

A

An alkali solution
React violently with water and more violent as you go down the group

64
Q

What do group 2 produce when they react with water

A

Produce hydroxides

65
Q

What do group 3456 metals produce when reacting with water

A

Nothing as they do not react
Transition metals react slowly with water and some do not react at all

66
Q

What metals can react with dilute acid

A

Metals above copper in the reactivity series can react with dilute acids to produce metal salts and hydrogen

67
Q

Why are reactions with calcium, strontium and barium more complicated when reacting with dilute acids

A

More complicates as the sulfates of these metals are insoluble which forms a protective layer that prevents more of the metals reacting

68
Q

Reactivity series

A

Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum

69
Q

Redox definition

A

Transfer of electrons during chemical reactions

70
Q

Reduction meaning

A

When electrons are gained

71
Q

Oxidation states meaning

A

The number assigned to an element in a chemical compound
It is a poitive or negative number depending on how many electrons the element has lost or gained

72
Q

Redox reaction meaning

A

Reactions in which atoms have changed their oxidation state changed

73
Q

How do you know if a reaction is not a redox reaction

A

If the oxidation states do not change

74
Q

A property of transitional metals

A

Have variable oxidation states due to their highest energy electrons being in the d sub shell
Good electrical and thermal conductors as they are malleable and ductile

75
Q

Use of a transition metal

A

Many are used as catalysts

76
Q

When will a metal displace a less reactive metal

A

In a metal salt solution

77
Q

Hwo does magnesium sulfate react with magnesium, zinc, iron and copper

A

No reaction

78
Q

How does zinc sulfate react with magnesium, zinc, iron and copper

A

Displacement for magnesium and rest no reaction

79
Q

How does iron sulfate react with magnesium, zinc, iron and copper

A

Displacement for magnesium and zinc
But rest iron and copper

80
Q

How does copper sulfate react with magnesium, zinc, iron and copper

A

No reaction for copper but rest displacement

81
Q

If halogens are oxidising agents what does this mean

A

They withdraw electrons from another atom/ion
The oxidising power of a halogen decreases as you go down group 7

82
Q

Does potassium chloride react with chlorine, bromine and iodine

A

No

83
Q

Does potassium bromide react with chlorine, bromine and iodine

A

Displacement with chlorine but rest no

84
Q

Does potassium iodine react with chlorine, bromine and iodine

A

No reaction with iodine but rest a displacement

85
Q

Applications and uses for metal and non-metal oxides

A

Magnesium oxide is used as a starter material for industrial processes such as producing magnesium alloys or fibreglass

86
Q

Application and uses for metal salts

A

Used to make the colours in fireworks

87
Q

Applications and uses of sodium chloride

A

Making glass, paper and rubber as well as being used in water softening systems

88
Q

Applications and uses of sulfates

A

Used in detergents

89
Q

Applications and uses of copper sulfate

A

Used in water treatment to kill algae

90
Q

Why does first ionisation energy increase across the period

A

As the number of protons increase across the period
Means that the force of attraction are pulling on the outer electrons increase

91
Q

What do extra protons increase and hiw foes the effect thr atomic radius

A

Increases the nuclear charge which attracts extra electrons pulling them closer to the nucleus

Science 2024 (10 decks)

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