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Btec Applied science > Chemistry Properties of substances > Flashcards

Chemistry Properties of substances Flashcards

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1
Q

What is a period ?

A

A period is a row in the periodic table

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2
Q

What do elements in the same period have ?

A

Elements in the same period have their valence electrons in the same shell

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3
Q

What is an example of a period in the periodic table ?

A

Magnesium and sulfur

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4
Q

What is a group in the periodic table ?

A

A group is a column in the periodic table.

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5
Q

What do elements in the same group have ?

A

Elements in the same group have their electrons in similar orbitals . They often have very similar properties

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6
Q

What is an example of a group in the periodic table ?

A

The halogens are all in group 7

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7
Q

Li, Be, B, C, N, O, F, Ne
What is this list of elements an example of?

A

A Period

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8
Q

What is the F block in the periodic table made up of ?

A

Lanthanides and Actinides

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9
Q

Which block would the transition metal tungsten lie in?

A

D

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10
Q

The ionisation of a species involves the removal of how many electrons?

A

1

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11
Q

What is Ionisation ?

A

Ionisation is the reaction where one electron is removed from an atom.

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12
Q

What is first ionisation energy ?

A

It is the energy required to remove an electron from every atom in a mole of atomic gas to produce a mole of unipostive gaseous ions

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13
Q

What is the second Ionisation energy ?

A

The secound Ionisation energy is the energy required to remove an electron from every ion of unipositive gaseous ions to produce a mole of dispositive gaseous ions.

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14
Q

What is the Third Ionisation energy ?

A

The third ionisation energy is the energy required to remove an electron from every ion in a mole of dispositive gaseous ions to produce a mole of trispostive gaseous ions.

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15
Q

The energy to remove an electron from X2+ is known as:

A

The third ionisation

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16
Q

What factors affect Ionisation energy and how ?

A

Electrons distance from nucleus - Greater distance decreases the Ionisation energy

Nuclear charge - Great nuclear charge increases the Ionisation energy

Shielding - More shielding electrons decrease the ionisation energy

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17
Q

What is shielding ?

A

shielding is where the increase in the number of electrons between the nucleus and outer electrons lead to the decrease in effective nuclear charge.

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18
Q

What are the trends in First Ionisation energies in the periodic table and why does it increase or decrease ?

A

First Ionisation energy increases across a period. This is because the atomic radius decreases .

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19
Q

In first ionisation energy Why does the Proton Number increase ?

A

Proton number increases across a period so electrons are more attracted to the nucleus. The electron is closer to the nucleus and so experiences a greater attraction. Nuclear charge increases across a period.

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20
Q

What happens to the trend in first ionisation energy down a group in the periodic table ? ( 6 MARKS)

A

It decreases down a group. This is because the atomic radius increases. The electron is further from the nucleus and so experiences lower attraction. There are also more electrons between the nucleus and the outer electrons. This means the outer electrons experience great shielding from the nucleus. This also provides evidence for the existence of shells.

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21
Q

Why does ionisation energy increase across a period?

A

Atomic radius is smaller and attraction is greater

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22
Q

What is the Periodic trend of the Atomic Radius ?

A

It decreases along a period.

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23
Q

Why does Atomic Radius decrease along a period in the periodic table ?

A

This is because the number of protons in the nucleus increases across the period. As you add protons , you also add electrons . Each electron feels a stronger attraction to the nucleus and is held closer.

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24
Q

Why does Atomic radius increase down a group in the periodic table ?

A

Atomic Radius increases down a group. This is because of the number of electron shells increases down a group. Each electron shell is further from the nucleus. This outweighs the increase in proton number down the group

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25
Why does the distance between electrons and nuclei increase down a group?
Valence electron shell gets bigger
26
What is Electronegativity ?
Electronegativity is the ability of an atom to attract a pair of electrons
27
What does Scaling Electronegativity mean ?
The elements have been scaled in terms of their electronegativity by the Pauling scale.
28
What does it mean when a molecule is polar ?
A molecule is polar if there is a charge separation between each side of the molecule.
29
A molecule contains multiple polar C-Cl bonds. Is the molecule definitely polar?
No - The polar bonds may cancel out.
30
Where are metals found on the periodic table ?
Metals are found on the left of the periodic table because they have few electrons in their outer shell.
31
What happens when metals react , what do they lose ?
When Metals react , they lose 1 or more of these negatively charged electrons to form positively charged ions.
32
33
Where are non - metals found on the periodic table ?
Non metals are found on the right of the periodic table because they have many electrons in their outer shell.
34
What happens when non metals react ?
When non-metals react they either gain electrons to form negatively charged ions or share electrons to form neutral molecules.
35
What are the Properties of Non - metals ?
They have lower melting and boiling points than metals. They are often found as gases. Non metals generally do not conduct heat or electricity
36
What are elements found in group 1 called ?
The Alkali Metals.
37
Facts about Lithium I need to Know ?
Lithium has the electron structure (2,1). Lithium is the least reactive of the alkali metals. Lithium burns with a crimson flame when it reacts with oxygen. Lithium floats on the surface of water and will release bubbles of hydrogen gas (it effervesces).
38
Facts about Sodium I need to know ?
Sodium has the electron structure (2,1). Sodium is more reactive than Lithium because its outer electron is less strongly attracted to the positively charged nucleus. This is because it is a greater distance from the positive charge of the atom's nucleus. The metal Sodium floats on the surface of water which releases enough heat to melt the sodium . The sodium moves quickly across the surface of the water. Sodium burns with a yellow/orange flame when it reacts with oxygen
39
Facts about Potassium I need to know ?
Potassium has the electron structure (2,1) Potassium is more reactive than lithium and sodium because its outer electron is least strongly attracted to the nucleus. The metal floats on the surface of water and has a similar but more vigorous reaction compared with sodium. Potassium burns with a Lilac flame when it reacts with oxygen.
40
What happens when alkali metals react with oxygen ?
The Metal rapidly turns from silvery shiny to dull as a metal oxide is produced
41
What happens when Alkali metals react with water ?
The Alkali metal floats on the surface and melts to create a metal hydroxide. When the alkali metals react with water the energy released is enough to melt the metal.
42
What happens when alkali metals react with chlorine ?
A metal chloride is formed which dissolves in water to give a colourless solution.
43
How many electrons do atoms of alkali metals have in their outer shell ?
1
44
Which alkali metal is not very reactive, burns with a crimson flame in oxygen and has the electron structure (2,1)?
Lithium
45
What is formed when alkali metals react with water?
Metal Hydroxide
46
Which colour flame would Lithium Produce when burned with Oxygen ?
Crimson or red flame
47
What are the uses of group 2 compounds ?
Titanium extraction As bases to neutralise acids In Healthcare Wet scrubbing
48
What is the melting point trend down Group 2 in the periodic table ?
Ion cores have larger radii down the group So, the free electrons experience less attraction to the nuclei . So, the bonding is weaker and the melting point is lower . Magnesium is the anomaly in Group 2
49
Why is calcium hydroxide (slaked lime) used on soil for growing crops?
It neutralises acidic soil to make it more favourable for crops to grow.
50
Why do the reactivity of group 2 metals increase down the group in the periodic table ?
Reactivity of group 2 metals increases down the group because the ionisation energies decrease. Increased shielding from more electron shells and a greater distance from the nucleus makes it easier to remove an electron from the outer shell.
51
How do group 2 oxides react with water?
Magnesium oxides react very slowly with water. Beryllium oxide does not react with water. Strontium oxide reacts with water steadily to produce metal hydroxide salts. Calcium oxide reacts steadily to produce metal hydroxide salts
52
What is Oxidation ?
Oxidation is Loss of electrons
53
What is Reduction ?
Reduction is Gain of electrons
54
What is an oxidising agent ?
An oxidising agent oxidises something else.
55
What do oxidising agents do ? ( 3 things)
It takes electrons from another compound. This means it gains electrons itself. An oxidising agent is itself reduced.
56
What is a reducing agent ?
A reducing agent reduce something else.
57
What do reducing agents do ? ( 3 things)
It gives electrons to another compound. This means it loses electrons itself. A reducing agent itself is oxidised.
58
What do Redox reactions involve ?
Redox Reactions involve the loss and gain of electrons
59
What does an oxidation state show ?
An oxidation state shows how many electrons an atom has gained or lost.
60
What is the oxidation state of oxygen ?
The Oxidation state of oxygen is always -2
61
When does the oxidation state of oxygen change ? ( 2 exceptions)
Unless you have a compound of oxygen and fluorine. The fluorine rule takes priority Another exception is in a peroxide
62
What is the oxidation state of Hydrogen ?
Hydrogen always has an oxidation state of +1
63
What is the 1 exception of the oxidation state of Hydrogen ?
Except in metal hydrides
64
What is the oxidation state for a compound ion ?
In a compound Ion the overall oxidation state is equal to the charge on the ion.
65
What is the oxidation state in a simple ion ?
In a simple ion, the oxidation state is just the charge on the ion.
66
What is the oxidation state in a pure element ?
In a pure element the oxidation state is zero.
67
How are Oxidation states represented ?
Oxidation states are commonly represented by Roman Numerals.
68
What is the oxidation state of Fe (ll)
+2
69
What does an Ionic half equation show ?
It shows either reduction or oxidation.
70
Two ionic half equations can be added together if what condition can be met ?
Equations for both reduction and oxidation
71
The co-ordination number of a complex is:
The number of dative bonds between a transition metal and its ligands
72
What are the metallic properties of transition metals ?
Conduct Electricity and heat Sonorous Hard Shiny
73
What is the observed colour change when iron (III) is reduced to iron (II)
From Brown to Green
74
What is a disproportionation reaction?
When an element is both oxidised and reduced in a reaction

Btec Applied science (5 decks)

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