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Chemistry OCR A-Level > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

How many electrons fill shell number 1?

A

2

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2
Q

How many electrons fill shell number 2?

A

8

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3
Q

How many electrons fill shell number 3?

A

18

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4
Q

How many electrons fill shell number 4?

A

32

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5
Q

What are shells regarded as?

A

energy levels

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6
Q

As the shell number increases, does energy increase or decrease?

A

increase

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7
Q

What is the principal quantum number, n?

A

shell number/energy level number

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8
Q

number of electrons =

A

2n²

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9
Q

What are shells made up of?

A

atomic orbitals

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10
Q

What is an atomic orbital?

A

1) region around the nucleus that can hold up to two electrons, with opposite spins
2) region in space where there is a high probability of finding an electron

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11
Q

What are the different types of orbitals?

A

1) s
2) p
3) d
4) f

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12
Q

Do each type of orbitals have the same or different shape?

A

different

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13
Q

In a s-orbital what shape is the electron cloud?

A

sphere

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14
Q

How many s-orbitals does each shell from n=1 contain?

A

1

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15
Q

In a s-orbital, the greater the shell number n, the…

A

greater the radius

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16
Q

In a p-orbital what shape is the electron cloud?

A

dumb-bell

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17
Q

How many electrons can an orbital hold?

A

1 or 2

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18
Q

How many p-orbitals does each shell from n=1 contain?

A

3

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19
Q

What angle are p-orbitals to one another?

A

right angles

20
Q

With a p-orbital, the greater the shell number n, the…

A

further the o-orbital is from the nucleus

21
Q

How many d-orbitals does each shell from n=1 contain?

A

5

22
Q

How many f-orbitals does each shell from n=1 contain?

A

7

23
Q

What charge do electrons have?

A

negative

24
Q

Do electrons attract or repel each other?

A

repel

25
Q

Which direction are electron spins?

A

up or down

26
Q

Do the two electrons in an orbital have the same or opposite spins?

A

opposite

27
Q

Why do the two electrons in an orbital have opposite spins?

A

to counteract the repulsion between the negative charges of the two electrons

28
Q

How can electron configurations be expressed more simply?

A

1) previous noble gas in the periodic table

2) outer shell electrons

29
Q

What are cations?

A

positive ions that are formed when atoms lose electrons

30
Q

What are anions?

A

negative ions formed when atoms gain electrons

31
Q

What is a s-block element?

A

highest energy electrons in s-sub-shell

32
Q

What is a p-block element?

A

highest energy electron in p-sub-shell

33
Q

What is a d-block element?

A

highest energy electron in d-sub-shell

34
Q

What is ionic bonding?

A

the electrostatic attraction between positive + negative ions

35
Q

What state are ionic compounds in at room temperature?

A

solid

36
Q

Why are ionic compounds solid at room temperature?

A

there is insufficient energy to overcome strong electrostatic forces of attraction between oppositely charged ions in giant ionic lattice

37
Q

Do ionic compounds have low or high melting and boiling points?

A

high

38
Q

What are the two main processes of solubility?

A

1) ionic lattice broken down

2) water molecules attract + surround ions

39
Q

When do ionic compounds conduct electricity?

A

1) once melted

2) once dissolved in water

40
Q

Why do ionic compounds not conduct electricity in the solid state?

A

1) ions in fixed position in giant ionic lattice

2) no mobile charge carriers

41
Q

Why do ionic compounds conduct electricity when liquid or dissolved in water?

A

1) solid ionic lattice breaks down

2) ions free to move as mobile charge carriers

42
Q

What is covalent bonding?

A

1) strong electrostatic attraction between a shared pair of electrons and nuclei of bonded atoms
2) overlap of atomic orbitals, each containing 1 electron, to give shared pair of electrons

43
Q

Between which atoms does covalent bonding occur?

A

1) non-metallic elements
2) compounds of non-metallic elements
3) polyatomic ions

44
Q

What are lone pairs?

A

paired electrons that are not shared

45
Q

What is a dative covalent/coordinate bond?

A

covalent bond in which shared pair of electrons is supplied by one bonding atom only

46
Q

What does average bond enthalpy measure?

A

covalent bond strength

Chemistry OCR A-Level (28 decks)

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