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Applied Science > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

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1
Q

What are Electron shells made up of

A

Sub-Shells

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2
Q

What are sub- shells made up of

A

Orbitals

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3
Q

How many electrons can an orbital hold

A

Two

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4
Q

What does a Nucleus contain

A

Protons and neutrons

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5
Q

What are the subatomic particles

A

Protons- Have a positive charge and found in the nucleus
Neutrons- Have no charge and found in the nucleus
Electrons- Have a negative charge and they orbit the nucleus int the shells

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6
Q

What is the atomic number?

A

The number of protons

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7
Q

What is the mass number?

A

Number of protons and neutrons

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8
Q

What is an isotope?

A

Same number of protons different number of nuetrons

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9
Q

How many electrons can shell 1, 2 and 3 hold?

A

Shell 1- 2 electrons
Shell 2- 8 electrons
Shell 3- 18 electrons

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10
Q

Describe S orbitals

A

Each energy level has one s-orbital
Can hold up to 2 electrons
Higher electron density near the nucleus
First two electrons of an atom will use this as its the lowest available energy level

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11
Q

Describe P orbitals

A

There are three p-orbitals in an energy level
Can hold up to 6 electrons

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12
Q

Describe D orbitals

A

At the third energy level there are five d-orbitals
Can hold up to 10 electrons

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13
Q

What order does the s, p, d orbitals go in?

A

1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p → 5s → 4d

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14
Q

What is ionic bonding?

A

A bond between a metal and a non-metal
Electrons are transferred

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15
Q

What happens during ionic bonding?

A

Metal atoms lose electrons to become positively charged ions called cations
Non-Metals gain electrons to become negatively charged ions called anions

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16
Q

What is an ionic bonding electrostatic attraction?

A

Attraction between oppositely charged ions

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17
Q

What are some ionic bonding properties?

A

High melting and boiling points
Conductive when molten or dissolved in water

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18
Q

What is covalent bonding?

A

Bond between non-metals where electrons are shared

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19
Q

What are the different types of covalent bonding?

A

Single bond-one pair of electrons shared
Double bond-two pairs of electrons shared
Triple bond-three pairs of electrons shared

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20
Q

What are some properties of covalent bonds?

A

Low melting and boiling points
Poor conductivity
Form molecules or giant covalent structures

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21
Q

What is metallic bonding?

A

Bonding in metals where electrons are delocalised

22
Q

What is the structure of metallic bonding?

A

Positive metal ions lost in ‘a sea of electrons’

23
Q

What are some of the properties of metallic bonding?

A

Good electric and thermal conductivity
Malleable
High melting and boiling points

24
Q

What is Van der Waals forces?

A

Weak forces between molecules which increase with molecular size

25
Q

What is Dipole-Dipole forces?

A

Attraction between polar molecules

26
Q

What is hydrogen bonding?

A

Strong intermolecular force when a hydrogen bond to highly electronegative atoms (N, O, F)

27
Q

Describe a diamond structure

A

Each carbon atom bonded to four others
Very hard
High melting point
Non-conductive

28
Q

Describe a graphite structure

A

Each carbon atom bonded to three others
Layers slide over each other
Conductive due to delocalised electrons

29
Q

Describe a silicone dioxide structure

A

High melting point
Found in sand and quartz

30
Q

What is electronegativity?

A

Tendency of an atom to attract atoms in a bond

31
Q

What is a polar bond?

A

Unequal sharing of electrons due to difference in electronegativity

32
Q

What is a non-polar bond?

A

Equal sharing of electrons

33
Q

What is the relative atomic mass (Ar)?

A

Weighted average mass of an element’s atoms compared to 1/12 the mass of a carbon-12 atom

34
Q

What is relative molecular mass (Mr)?

A

Sum of relative atomic masses of all atoms in a molecule

35
Q

How do you calculate the Mr?

A

the sum of the relative atomic masses of the atoms in the numbers shown in the formula

36
Q

What is a Mole?

A

Unit of amount of substance in chemistry; 1 mole = 6.022×10’23 particles (Avogadro’s constant).

37
Q

What is the molar mass (g/mol)?

A

Mass of 1 mole of a substance
Equal to the Mr

38
Q

What is the formula to find Moles?

A

Number of moles = mass (g) / molar mass (g/mol)

39
Q

How do you convert moles to particles?

A

Particles = moles × Avogadro’s constant

40
Q

How do you calculate the mass?

A

Mass (g) = moles × molar mass

41
Q

What is the formula to calculate the volume of gases?

A

Volume (dm³) = moles × 24

42
Q

What is the formula for concentration?

A

Concentration (mol/dm³) = moles / volume (dm)

43
Q

What equation contains moles, concentration and volume?

A

Moles = concentration (mol/dm³) × volume (dm³)

44
Q

What is the empirical formula?

A

Simplest whole-number ratio of atoms in a compound
Find by dividing moles of each element by the smallest mole value

45
Q

What is the molecular formula?

A

Actual number of atoms of each element in a molecule
Find by multiplying the empirical formula by a whole number so the molar mass matches the molecular mass

46
Q

How do you balance an equation?

A

Make the same number of each type of atom on both sides of the equation
Write the unbalanced equation.
Balance each element one at a time, adjusting coefficients.
Double-check for equal atoms on each side.

47
Q

What is the percentage yield?

A

Measures efficiency of a reaction

48
Q

What is the formula for percentage yield?

A

PercentageYield= theoreticalyield/ actualyield×100%

49
Q

What is the actual yield?

A

Mass obtained from the experiment

50
Q

What the theoretical yield?

A

Mass calculated based on stoichiometry

51
Q

What factors affect yield?

A

Incomplete reactions
Side reactions
Losses during recovery

Applied Science (6 decks)

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