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Applied Science Unit 1 Chemistry > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

Understand all types of atom's bonds and structure

You may prefer our related Brainscape-certified flashcards:
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1
Q

How many electrons can an s subshell hold?

A

2

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2
Q

How many electrons can a p subshell hold?

A

6

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3
Q

How many electrons can a d subshell hold?

A

10

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4
Q

How many electrons can a f subshell hold?

A

14

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5
Q

What is Aufbau principle?

A

Electrons always inhabit the lowest energy orbitals available

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6
Q

Electrons repel each other so what holds them together and why?

A

Spin creates magnetism (moving charge)

Opposite spin creates opposite magnetic fields

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7
Q

What is does electronegativity mean?

A

How attractive a nucleus is to electrons

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8
Q

What are the properties that affect electronegativity?

A

Larger charge=more attractive

Charge density, more neutrons “dilute” positive charge =lower attractive

Inner electrons shield outer electrons reduces attraction

Distance, the further away, the weaker the attraction

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9
Q

What is the most electronegativity element

A

Fluorine

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10
Q

Why does ionic bonding occur?

A

Because the non-lethal has higher electronegativity so it steals electrons from the metal

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11
Q

Why does convent bonds occur?

A

Similar electronegativity so they share electrons instead of stealing

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12
Q

Why does metallic bonding occur?

A

Same electronegativity so they share electrons between the positive nucleuses
Delocialised electrons

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13
Q

What happens to electronegativity across periods?

A

Adds protons so it increases

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14
Q

What happens to electronegativity down groups?

A

More distance and more shielding so decreasing electronegativity

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15
Q

What is stoichiometry?

A

The ratios of reactants

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16
Q

What is promotion and why is it important?

A

Promotion is when electrons from 2s^2 move to 2p orbit
Promotion explains how carbon bond makes colavent bonds as it means a sub shell is freed up for an electron to bond

A mixture of s, p electrons forming a bond

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17
Q

Ionic electron clouds look like

A

Cloud is more around the highly electronegative atom because more attractive to electrons

One side is denuded of electrons

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18
Q

Colavent electron clouds look like

A

Even spread as similar electronegativities

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19
Q

What are the 3 types of Van der Waals forces

A

Hydrogen bonding

London dispersion forces (temporary dipoles)

Permanent dipoles

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20
Q

What are Van Der Waals forces

A

Weak attractive forces between molecules

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21
Q

What is a tetrahedron and what angle between pairs?

A

The shape a molecule forms with one central atom and 4 bonded atoms

109.47°

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22
Q

How do London dispersion forces work?

A

Electrons repel each other to create temporary positive charge in the charge cloud
The charged bits are then attracted to each other

23
Q

What is the order of strength of Van Der Waals forces?

A

Hydrogen
Permanent dipoles
London dispersion forces

24
Q

How do you work out moles?

A

Moles = Mr/Mass

25
Q

What order do the orbital go in?

A

S, p, d, f

26
Q

How do you calculate molar mass?

A

Mass/moles

27
Q

How do you calculate concentration?

A

Moles/volume

28
Q

What are the uses for magnesium oxide?

A 
Fertilizer
Mineral supplement
Ice control
Dust control
Coagulant for making food
Spa treatment
29
Q

Explain why copper is ductile?

A

Metallic bonding means a regular pattern

This means atoms can slip past each other easily

So metals can be drawn into wires without breaking

30
Q

Balance equation for the reaction of silicon and oxygen

A

Si + O^2 –⟩ SiO^2

31
Q

What is the force called between ions?

A

Electrostatic force

32
Q

What is the formulae of hydroxide?

A

OH-

33
Q

What is the formulae of carbonate

A

CO3²-

small low 3

34
Q

What is the formulae of sulphate

A

SO4²-

small low 4
small high 2

35
Q

What is the formulae of nitrate

A

NO3-

small low 3

36
Q

What is the formulae of ammonium

A

NH4+

small low 4

37
Q

How do you work out molarity?

A

Molarity= moles/ litres of solution

38
Q

What is Aufbau principle?

A

Electrons will fill the orbital with the lowest available energy state

39
Q

What intermolecular forces do noble gases have?

A

London dispersion forces

40
Q

How do you work out percentage yield with moles?

A

Actual number of moles/expected number of moles *100

41
Q

What is an element?

A

A substance made from one type of atom

42
Q

What is a quantum?

A

A quantum is how much energy an electron needs to move to the next energy level

Losing energy is dropping a level
Gaining energy is moving up a level

43
Q

What’s important to remember when drawing calcium electron configuration which has 20 electrons?

A

4s fills in before 3d

44
Q

What is the structure of ionic compounds?

A

Lattice giant structure usually regular pattern

45
Q

What does the strength of an ionic bond depend on?

A

More charge means more electrostatic forces

Smaller ionic radius electrons are closer to the nucleus

46
Q

What is a dative bond?

A

Where the electrons come from the same atom, Colavent bond

47
Q

What affects the strength of covalent bonds

A

Shorter covalent bonds on a stronger closer to the nucleus

Multiple bonds are stronger

48
Q

Why are metals good conductors of heat?

A

At higher temperatures metal atoms vibrate more. Bypass this vibration energy (kinetic/heat) to their neighbours

Free electrons carry energy through the metals

49
Q

Why are metals good conductors of electricity?

A

Electrons are delocalized and negatively charged

Free electrons can move through the metal and current is the flow of charge

50
Q

Why does the melting point decrease as we go down metals groups?

A

The atoms of bigger as they have more shells

The distance between the nucleus and the delocalized electrons are bigger

The forces holding the structure together are weaker

51
Q

What are inter-molecular forces and their name?

A

The forces between molecules

Van de Waals forces

52
Q

Why are elements put into groups?

A

Put into groups of similar properties

53
Q

How many elements is there?

A

92

54
Q

What is electron affinity and what is it measured in?

A

How likely a neutral atom is to gain an electron

Measured in the energy released Kj/mol

Applied Science Unit 1 Chemistry (3 decks)

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