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Chemistry Module 2 > Chapter 5: Electrons and Bonding > Flashcards

Chapter 5: Electrons and Bonding Flashcards

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1
Q

What are shells regarded as?

A

energy levels

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2
Q

What is the energy level called and made up of ?

A

The principal quantum number (n)
atomic orbitals

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3
Q

How many electrons can fill the first energy level?

A

2

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4
Q

How many electrons can fill the second energy level?

A

8

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5
Q

How many electrons can fill the third energy level?

A

18

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6
Q

How many electrons can fill the fourth energy level?

A

32

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7
Q

What is an atomic orbital?

A

a region in space where there’s a higher probability of finding an electron and it contains a maximum of two electrons with opposite spins

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8
Q

Name the types of orbitals in order

A

s orbitals
p orbitals
d orbitals
f orbitals

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9
Q

What is the shape of an s orbital?

A

Spherical

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10
Q

What is the shape of a p orbital?

A

dumbbell

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11
Q

How many sub shells make up s orbital?

A

one

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12
Q

How many electrons can fill the sub shells in s orbital?

A

2

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13
Q

How many sub shells make up p orbital?

A

3

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14
Q

How many sub shells make up d orbital?

A

5

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15
Q

How many electrons can fill the sub shells in p orbital?

A

6

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16
Q

How many electrons can fill the sub shells in d orbital?

A

10

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17
Q

What are the subshells for orbitals in energy level 1?

A

1s

18
Q

What are the subshells for orbitals in energy level 2?

A

2s + 2p

19
Q

What are the subshells for orbitals in energy level 3?

A

3s + 3p + 3d

20
Q

What are the subshells for orbitals in energy level 4?

A

4s + 4p + 4d + 4f

21
Q

What is the order of filling shells in n=2?

A

2s then 2p

22
Q

What is the order of filling shells in n=3?

A

3s then 3p then 3d

23
Q

What is the order of filling shells in n=4?

A

3p then 4s then 3d

24
Q

How do you fill orbitals with the same subshell?

A

fill each orbital of a p sub shell with one electron before pairing

25
Q

How is an electron spin shown on ‘Electron in box’ model?

A

an arrow up or down

26
Q

Why must electrons have opposite spins?

A

to counteract the repulsion between the negative charges of the electrons

27
Q

Show the electronic configuration of Z=36 (Krypton)

A

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6

28
Q

What is ionic bonding?

A

The electrostatic attraction between positive and negative ions

29
Q

What is the structure of ionic compounds?

A

Giant ionic lattice due to oppositely charged ions strongly attracted in all directions

30
Q

Why do ionic compounds have high melting and boiling points?

A

high temperatures are needed to provide the large quantity of energy to overcome the strong electrostatic attraction between the ions.

31
Q

Why do ionic substances dissolve in water?

A

because water is polar and stabilises the separated ions by surrounding the ions

32
Q

Why do ionic substances conduct electricity when aqueous?

A

ions are free to move and conduct

33
Q

Why don’t ionic substances conduct electricity when solid?

A

ions are held strongly in a lattice

34
Q

What does 1st Ionisation energy mean?

A

The energy required to remove one mole of electrons from one mole of gaseous atoms
X(g) —> X^+(g) + e

35
Q

What does electron affinity mean?

A

The energy when one mole of gaseous atoms acquires one mole of electrons to form one mole of gaseous negative ions

36
Q

What is a covalent bond?

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

37
Q

What is a dative/coordinate covalent bond?

A

When the shared pair of electrons has been supplied by one of the bonding atoms only

38
Q

What does average bond enthalpy mean?

A

a measurement of covalent bond strength

39
Q

What are the three most electronegative elements?

A

F, N, O

40
Q

What is an oxidising agent?

A

an element that takes the electrons from the element being oxidised

41
Q

Where is the s, p and d block on the periodic table?

A

s block = left two groups
p block = right six groups
d block = centre groups

42
Q

Why would Na2S have a higher melting temperature than NaCl

A

Na2S = sulphur has 2-
NaCl = chlorine has 1-

Na2S has stronger ionic bonds due to the higher charge therefore more energy is needed to overcome bonds

Chemistry Module 2 (2 decks)

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