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Unit One: Chemistry > Unit One > Flashcards

Unit One Flashcards

1
Q

What is a covalent bond between?

A

A covalent bond is between two non metals

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2
Q

What happens to electrons in a covalent bond?

A

They share electrons.

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3
Q

What is the structure for covalent bonds?

A

Either small molecules or giant lattices.

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4
Q

Give examples of covalent bonds.

A
  • H2O,
  • H2,
  • O2,
  • NH4
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5
Q

What is ionic bonds between?

A

A ionic bond is between a metal and a non-metal.

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6
Q

What happens to electrons in ionic bonding?

A

The metal loses electrons and forms positive ions.

The non-metal gains electrons and forms negative electrons.

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7
Q

What is the structure for ionic bonds?

A

Giant lattices.

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8
Q

Give examples of ionic bonds.

A
  • CaO
  • LiCl
  • MgBr2
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9
Q

What is metallic bonding?

A

Metallic bonding is the attraction between positive metal ions and delocalised electrons.

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10
Q

Describe the structure of metals.

A
  • Regular row or positive ions
  • Metal ions
  • Sea of delocalised electrons
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11
Q

Describe the properties of metals.

A
  • Conducts electricity & heat
  • High melting & boiling point
  • Ductile / Malleable
  • Some are catalysts
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12
Q

Why are metals good conductors?

A

They have electrons which are delocalised so they can move and they carry a charge.

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13
Q

Why do metals have high melting points?

A

There is a strong electrostatic force between the sea of delocalised electrons and the cations (positive metal ions) therefore it requires a large amount of energy to break the bonds.

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14
Q

Why are metals ductile / malleable?

A

The layers of positive ions can slide over each other.

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15
Q

What does ductile mean?

A

They can be pulled out into wires.`

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16
Q

What does malleable mean?

A

They can be shaped into sheets.

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17
Q

What is the equation for moles? (Molar mass)

A

Moles = Mass (g) / Molar mass (g/mol)

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18
Q

What is molar mass?

A

The larger number on the periodic table.

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19
Q

What is the equation for concentration?

A

Concentration = Moles (mol) / Volume (dm3)

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20
Q

What is the units for concentration?

A

Mol/dm3

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21
Q

Whats is Avogadro’s constant?

A

6.023 x 10^23

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22
Q

What is the chemical formula for Sulphate?

A

SO4^-2

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23
Q

What is the chemical formula for Nitrate?

A

NO3^-1

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24
Q

What is the chemical formula for Hydroxide?

A

OH^-1

25
Q

What is the chemical formula for Carbonate?

A

CO3^-2

26
Q

How many electrons can fit in a S orbital?

A

Only 2 electrons can fit on a S orbital.

27
Q

How many P orbitals are grouped together?

A

P orbitals come in sets of 3.

28
Q

How many D orbitals are grouped together?

A

D orbitals come in sets of 5.

29
Q

What’s the maximum amount of electrons in P orbitals?

A

You can have a maximum amount of 6 electrons.

30
Q

What’s the maximum amount of electrons in D orbitals?`

A

You can have a maximum amount of 10 electrons

31
Q

What is the order that the orbitals fill?

A

1S, 2S, 2P, 3S, 3P, 4S, 3D, 4P, 4D, 4F

32
Q

If a volume is in cm3 what do you do?

A

Divide the volume by 1000 to convert it to dm3

33
Q

Why are some metals catalysts?

A

Some metals are catalysts due to their variable charges.

34
Q

What are isotopes?

A

Isotopes are elements with the same number of protons but different number of neutrons.

35
Q

What is the equation for isotopes?

A

((Mass of isotope 1 x percentage) + (Mass of isotope 2 x percentage)) / 100

36
Q

What is Electronegativity?

A

The ability of an atom to attract the bonding pair of electrons in a covalent bond.

37
Q

If an element has a larger electronegativity value, what does this mean?

A

The larger the value, the larger the ability of the element to attract thr pair of electrons from a covalent bond.

38
Q

What happens to the values of electronegativity when you go down a group?

A

The values decrease.

39
Q

What happens to the value of electronegativity when you go across a period?

A

The values increase.

40
Q

What effect does the nuclear charge have on the electronegativity value?

A

The greater the nuclear charge, the greater the electronegativity of the element because the element contains a greater number of protons to attract the electrons.

41
Q

What is a dative covalent bond?

A

When one atom gives both electrons that are shared. The other atom must have room to receive both.

42
Q

What is an example of dative covalent bonding?

A

NH4 - Ammonium ion

43
Q

What is a standard solution?

A

A standard solution is a solution that contains a precisely known concentration of an element or substance.

44
Q

What does polar mean?

A

It means that between two elements, there are more electrons at one side therefore one side is more negative.

45
Q

What does non-polar mean?

A

The electron cloud is evenly distributed. The atoms attract the electron pair equally so it’s equally paired.

46
Q

What effect does the atomic radius have on the electronegativeity value?

A

The greater the atomic radius, the lower the electronegativity value. This is because there is a shielding effect from the inner electron shells. The greater the number of shells, the greater the shielding effect.

47
Q

Is H-H polar or non-polar?

A

Non-polar as it has en equal amount of electrons.

48
Q

Is O-H polar or non polar?

A

Polar as oxygen has a larger amount of electrons.

49
Q

What is the most electronegative element?

A

Fluorine

50
Q

What is the weakest intermolecular force?

A

Van de waals / London forces are the weakest forces because they are only temporary.

51
Q

What are the only elements hydrogen bonding can occur in?

A
  • Oxygen
  • Nitrogen
  • Fluorine
52
Q

Why can hydrogen bonding only occur in certain elements?

A
  • Those elements have the biggest difference in electronegativity.
53
Q

What molecules can endure Van de Waals / London forces?

A

All molecules.

54
Q

When does a dipole-dipole interaction occur?

A

Dipole-dipole interactions can only take place when there is a polar molecule.

55
Q

Why does Br2 have a stronger Van de Waal bond compared to Cl2?

A

Bromide is a larger molecule.

56
Q

What is a temporary dipole?

A

Random electron movement.

57
Q

What is Van de waals forces?

A

It is when a temporary dipole induces a nearby molecule.

58
Q

When is Van de Waals forces strongest?

A

In larger molecules.

59
Q

What are intermolecular forces?

A

Intermolecular forces are forces between molecules which determine the boiling point due to polar interactions.

Unit One: Chemistry (2 decks)

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