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C2 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

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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

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3
Q

Characteristics for period 3

A

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

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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

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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

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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

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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

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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

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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

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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

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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

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12
Q

Cations meaning

A

Ions with a positive charge

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13
Q

Isoelectronic meaning

A

Having the same number of electrons

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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

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15
Q

Anions

A

Ions with a negative charge

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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

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17
Q

Electronegativity

A

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

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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

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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

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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

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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

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22
Q

First ionisation energy

A

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

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23
Q

Periodicty

A

The repeating pattern seen by the elements in the periodic table

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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

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25
Why is it harder to remove an electron as you go across a period
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
26
Electron affinity
The change in energy when one mole of gaseous atoms gains one mole of electrons to form a mole of negative ion
27
What are the elements that are included in the first electron affinity
Fluorine, chlorine bromine and iodine
28
What are first electron affinities
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.
29
What is the first electron affinity for fluorine
-328
30
What is the first electron affinity for chlorine
-349
31
What is the first electron affinity for bromine
-324
32
What is the first electron affinity fot iodine
-295
33
What does electron affinity indicate for group 7
How strong the attraction is between the nucleus of an atom and the incoming electron if this attraction is strong more energy is released
34
What has an effect on electron affinity
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
35
Why does fluorine not follow electron affinity pattern
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
36
How is group 6 similiar to group 7s electron affinity
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
37
What can be used to predict the type of bonding in a compound
Electronegativity
38
Can you directly measure electronegativity of an element
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
Qhat does it mean if the electronegativities of the elements forming bonds are low
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
How do ionic bonds show polarity
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
What do melting and boiling points depend on
The strength of the forces between the atoms in an element
42
What is the melting ang boiling point going down group 1 and 7
Decreases which means the forces of attraction are weaker And Increases which means stronger
43
How will u get a high melting and boiling point
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
What happens when you go across period 1 to 3
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
Why does carbon have a high melting and boiling point
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
Why does sulfur have a higher melting and boiling pointthan the rest of non metals in period 3
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
What bond has the best for electrical conductivity
Copper and metallic bonding which allows electrical conductivity through a solid or liquid metal
48
What do delocalised electrons do in electrical conductivity and why are they good
Carry the electrical charge and absorb heat energy which gives them kinetic energy. This energy is transferred through the metal by these electrons
49
Are metals good thermal conductors malleable and ductile
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
Chemical properties of element example
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
How does group 1 elementa react with oxygen
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
How does group 2 elements react with oxygen
Beryllium and magnesium Needs hat to reach as to do with group 1 elements and very vigorous reactions
53
How does group 3 elements aluminium react with oxygen
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
How does group 4 carbon and silicon react with oxygen
Forms slightly acidic oxides that shows reaction with heat but no reaction
55
How does group 5 elements nitrogen and phosphorus react with oxygen
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
How does group 6 elements oxygen and sulfur react with oxygen
In ozone layer Two oxides form Burns slowly with blue flame
57
How does group 7 elements e.g halogens react with oxygen
Unstable oxides form
58
How does group 0 elements neon and argon react with oxygen
No reaction
59
Alkaline solution meaning
A solution with a pH above 7
60
Oxidisation meaning
Loss of atoms/electrons
61
Allotropes meaning
Two or more different physical forms that an element can exist in
62
Amphoteric meaning
Substance that can act as both an acid and a base
63
When group 1 reacts with water what do they produce
An alkali solution React violently with water and more violent as you go down the group
64
What do group 2 produce when they react with water
Produce hydroxides
65
What do group 3456 metals produce when reacting with water
Nothing as they do not react Transition metals react slowly with water and some do not react at all
66
What metals can react with dilute acid
Metals above copper in the reactivity series can react with dilute acids to produce metal salts and hydrogen
67
Why are reactions with calcium, strontium and barium more complicated when reacting with dilute acids
More complicates as the sulfates of these metals are insoluble which forms a protective layer that prevents more of the metals reacting
68
Reactivity series
Potassium Sodium Calcium Magnesium Aluminium Carbon Zinc Iron Tin Lead Hydrogen Copper Silver Gold Platinum
69
Redox definition
Transfer of electrons during chemical reactions
70
Reduction meaning
When electrons are gained
71
Oxidation states meaning
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
Redox reaction meaning
Reactions in which atoms have changed their oxidation state changed
73
How do you know if a reaction is not a redox reaction
If the oxidation states do not change
74
A property of transitional metals
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
Use of a transition metal
Many are used as catalysts
76
When will a metal displace a less reactive metal
In a metal salt solution
77
Hwo does magnesium sulfate react with magnesium, zinc, iron and copper
No reaction
78
How does zinc sulfate react with magnesium, zinc, iron and copper
Displacement for magnesium and rest no reaction
79
How does iron sulfate react with magnesium, zinc, iron and copper
Displacement for magnesium and zinc But rest iron and copper
80
How does copper sulfate react with magnesium, zinc, iron and copper
No reaction for copper but rest displacement
81
If halogens are oxidising agents what does this mean
They withdraw electrons from another atom/ion The oxidising power of a halogen decreases as you go down group 7
82
Does potassium chloride react with chlorine, bromine and iodine
No
83
Does potassium bromide react with chlorine, bromine and iodine
Displacement with chlorine but rest no
84
Does potassium iodine react with chlorine, bromine and iodine
No reaction with iodine but rest a displacement
85
Applications and uses for metal and non-metal oxides
Magnesium oxide is used as a starter material for industrial processes such as producing magnesium alloys or fibreglass
86
Application and uses for metal salts
Used to make the colours in fireworks
87
Applications and uses of sodium chloride
Making glass, paper and rubber as well as being used in water softening systems
88
Applications and uses of sulfates
Used in detergents
89
Applications and uses of copper sulfate
Used in water treatment to kill algae
90
Why does first ionisation energy increase across the period
As the number of protons increase across the period Means that the force of attraction are pulling on the outer electrons increase
91
What do extra protons increase and hiw foes the effect thr atomic radius
Increases the nuclear charge which attracts extra electrons pulling them closer to the nucleus

Science 2024 (10 decks)

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