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Z. Higher Chemistry > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

How are elements on the periodic table arranged?

A

Elements on the periodic table are arranged by increasing atomic number.

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2
Q

What does the position of elements on the periodic table allow us to predict?

A

The position of elements on the periodic table allow chemists to make predictions of their physical properties and chemical behaviour.

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3
Q

What happens as you go down a group in the periodic table regarding electrons?

A

Going down in a group on the periodic table, the elements contain the same number of outer electrons but an extra outer election shell each time.

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4
Q

What happens to the state of elements as you move along a period?

A

Going along a period elements move from metallic to non-metallic and add an outer electron each time.

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5
Q

What of the first 20 elements in the periodic table are metallic lattices?

A 
Li
Be
Na
Mg
Al
K
Ca
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6
Q

What are the first 20 elements in the periodic table are covalent molecular

A 
H2
N2
O2
F2
Cl2
P4
S8
Fullerenes (e.g. C60)

‘Some People Never Have Other Fresh Clothes’ + fullerenes

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7
Q

What is the first 20 elements in the periodic table are covalent networks

A

B
C (diamond, graphite)
Si

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8
Q

What is the first 20 elements in the periodic table are monatomic

A

Noble gases

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9
Q

Covalent radius meaning

A

The covalent radius as a measure of the size of an atom.

It is defined as half the distance between the nuclei of two bonded atoms.

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10
Q

What happens to the covalent radius across a period?

A

Across a period, the covalent radius decreases because of increased nuclear charge (electrons are attracted closer to the nucleus).

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11
Q

What happens to the covalent radius going down a group?

A

Going down a group, the covalent radius increases as the number of occupied electron shells increases

(More shells = bigger atom)

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12
Q

First ionisation energy definition

A

The first ionisation energy is the energy required to remove one mole of electrons from one mole of atoms in the gaseous state.

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13
Q

Second ionisation energy definition

A

The second ionisation energy is the energy required to remove the second more of electrons in the gaseous state.

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14
Q

What happens to the ionisation energy across a period

A

Across a period that ionisation energy increases because of increased nuclear charge. (So more energy is required to remove 1 mole of electron)

(Greater pull on the electrons so more energy required to remove them)

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15
Q

What happens to the ionisation energy going down a group

A

Down a group, ionisation energy decreases because of increased electron shells which means there is an increased shielding affect due to the inner electrons.

(Held less strongly so less energy required to remove the electron)

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16
Q

Electronegativity definition

A

Electronegativity is a measure of an atoms attraction for the shared pair of electrons in a bond.

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17
Q

What happens to the electronegativity values across a period

A

Across a period, electronegativity increases because of increased nuclear charge (attracting the electrons more strongly to the nucleus so more energy is required to remove one mole of electron)

(Greater nucleus charge and therefore a smaller covalent radius across a group which allows an atoms nucleus to have a greater force of attraction for electrons.)

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18
Q

What happens to electronegativity values down a group

A

Going down a group, electronegativity decreases due to the screening affect. (As a result of shielding and the increased covalent radius the outer electron requires less energy to be removed).

(Inner electrons will shield the nuclear charge)

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19
Q

What usually forms a covalent bond

A

A covalent bond usually occurs between non-metal elements.

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20
Q

What is a covalent bond

A

A covalent bond is an electrostatic force of attraction between positively charged nuclei and a shared pair of negatively charged outer electrons.

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21
Q

When are polar covalent bonds formed

A

Polar covalent bonds are formed when the (different) atoms attractions for the pair of bonding electrons are different.

(They have different electronegativity values)

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22
Q

What happens to charges on atoms when polar covalent bonding occurs

A

One atom will become delta positive and the other delta negative.

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23
Q

What atoms becomes Delta negative in polar covalent bonding

A

The atom with the higher electronegativity will be delta negative because it has a stronger attraction for negatively charged electrons

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24
Q

Are all substances with polar covalent bonds polar molecules?

A

Not all substances with polar covalent bonds will be polar molecules.

If a molecule that has polar bonds has a symmetrical arrangement it will be nonpolar because the overall polarity cancels out

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25
Q

Polar molecules Vs nonpolar molecules

A

Polar molecules are molecules that contain polar bonds and are asymmetric.

Non-polar molecules may contain polar bonds but they are symmetrical so the overall polarity cancels out.

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26
Q

Describe the bonding continuum

A

The bonding continuum shows the continuum of states from covalent to ionic bonds

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27
Q

What is the state of covalent networks at room temperature

A

Solid

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28
Q

What is the state of covalent molecular at room temperature

A

Gas or liquid

29
Q

What is the state of ionic substances at room temperature

A

Solid

30
Q

Describe the melting point of covalent molecules

A

Low melting point

31
Q

Describe the melting point of covalent network

A

Very High melting points

32
Q

Describe the melting point of ionic bonds

A

High melting points

33
Q

What is the relationship between solubility and molecular size

A

Solubility decreases as molecular size increases

34
Q

Are polar covalent Compounds and ionic substances soluble in water

A

Polar covalent compounds and ionic substances tend to be soluble in water.

(Remember ‘like dissolves like’)

35
Q

Do covalent bonds conduct electricity

A

Covalent bonds do not conduct electricity except for carbon in the form of graphite

36
Q

Do ionic bonds conduct electricity

A

Ionic bonds can conduct electricity when molten or in solution

37
Q

What are intermolecular forces

A

Intermolecular forces act between molecules. These are known as van Der waals forces.

38
Q

State intermolecular forces (3)

A

London dispersion forces

Permanent dipole- permanent dipole attractions

Hydrogen bonding

39
Q

Where does London dispersion forces exist and what is their strength

A

London dispersion forces are the weakest form of intermolecular bonding and the exist between all atoms and molecules

40
Q

What causes dispersion forces

A

Dispersion forces are caused by uneven distribution of electrons

41
Q

What forms London dispersion forces

A

London dispersion forces are formed by the electrostatic attraction between temporary dipoles and induced dipoles which are caused by the movement of electrons in atoms and molecules.

42
Q

What makes a London dispersion force stronger

A

London dispersion forces get stronger when there are more electrons in an atom/molecule

43
Q

Why do all molecules and atoms contain London dispersion forces

A

They all contain London dispersion forces because they all have electrons

44
Q

When are molecules described as polar

A

Molecules are polar when they have a permanent dipole (one end of molecule is permanently positive, other permanently negative)

45
Q

What are permanent dipole-permanent dipole attractions

A

Permanent dipole-permanent dipole attractions are the intermolecular force of attraction between oppositely charged ends of the polar molecules.

46
Q

Are permanent dipole permanent dipole interactions stronger than London dispersion forces

A

Permanent dipole permanent dipole interactions are stronger than London dispersion forces

47
Q

What are permanent dipole permanent dipole attractions in addition to

A

Parent dipole permanent dipole attractions between molecules are in addition to London dispersion forces.

48
Q

What are hydrogen bonds

A

Hydrogen bonds are permanent dipole – permanent dipole interactions found between molecules which contain highly polar bonds

(They are electrostatic forces of attraction between molecules that contain highly polar bonds) - 3 elements

49
Q

What can hydrogen bonds form between

Elements, 3

A

They are usually found in molecules where hydrogen is bonded to very electronegative atoms.

Hydrogen - FLUORINE
Hydrogen- NITROGEN
Hydrogen- OXYGEN

50
Q

What are the strongest intermolecular force

A

Hydrogen bonds are the strongest intermolecular force

51
Q

Compare the strength of hydrogen bonds to permanent dipole permanent dipole attractions and London dispersion forces and covalent bonds

A

Hydrogen bonds are stronger than permanent dipole permanent dipole attractions and London dispersion forces but weaker than covalent bonds.

52
Q

Describe how intermolecular forces of attraction affect a molecules physical properties

A

As the strength of the intermolecular force of attraction increases, so does melting and boiling point and viscosity.

53
Q

Why does ammonia on water have high boiling points

A

Ammonia on water have high boiling points due to hydrogen bonding

54
Q

What usually dissolves polar molecules

A

Polar solvents will usually dissolve polar molecules

‘Like dissolves like’

55
Q

What usually dissolves nonpolar molecules

A

‘Like dissolves like’

Nonpolar solvents will usually dissolve nonpolar molecules

56
Q

What type of solvent as water

A

Water is a polar molecule so it is a polar solvent

57
Q

What do ionic lattices and polar covalent molecular compounds tend to be soluble in?

A

Ionic lattices and polar covalent molecular compounds tend to be

soluble in water and other polar solvents, due to the attraction between the opposite charges.

58
Q

What do ionic lattices and polar covalent molecular compounds tend to be soluble in?

A

Ionic lattices and polar covalent molecular compounds tend to be

Insoluble in nonpolar solvents, as there is no attraction between the ions and the solvent molecules.

59
Q

Reduction & oxidation definition

A

Reduction is gain of electrons by a reactant (or loss of oxygen).

Oxidation is loss of electrons by a reactant (or gain of oxygen).

OIL RIG

60
Q

Redox reaction definition

A

A Redox Reaction is when an oxidation and a reduction reaction takes place at the same time.

61
Q

What is an Oxidising agent

A

Oxidising agent is a substance that accepts electrons (helps another reactant to be oxidised by being reduced itself).

62
Q

What is a reducing agent

A

Reducing agent is a substance that donates electrons (helps another reactant to be reduced by being oxidised itself).

63
Q

Recognising oxidising and reducing agents

A

Elements with low electronegativities can form ions by losing electrons so act as reducing agents (elements with high electronegativities can act as oxidising agents).

Strongest reducing agents are in Group 1 of the Periodic Table (strongest oxidising agents are in Group 7).

64
Q

Oxidising agents location on PT and examples

A

Oxidising agents are at the bottom of the left-hand side column of the electrochemical series:

permanganate (MnO4-)
dichromate (Cr2O72-)
hydrogen peroxide (H2O2)

65
Q

Reducing agents location on PT

A

Reducing agents are at the top right-hand column of the electrochemical series.

66
Q

Oxidising agent uses

A

Oxidising agents can be used to kill fungi and bacteria and also as a bleach.

67
Q

Metallic properties

A

Metallic elements can conduct electricity in any state.

This is because they have delocslised electrons (free to move).

68
Q

Metallic bond definition

A

A metallic bond is the electrostatic force of attraction between positively charged ions and delocalised electrons.

Z. Higher Chemistry (4 decks)

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