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physchem > O7s > Flashcards

O7s Flashcards

1
Q

Define Atomic Number?

A

Atomic number is the number of protons.

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2
Q

Define Mass Number?

A

Mass number is the number of protons and neutrons.

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3
Q

Define a Mole?

A

A mole is 6 x 10^23, Avogadro’s number.

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4
Q

What is the shape of the s orbital?

A

Sphere.

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5
Q

What is the shape of a p orbital?

A

Dumbbell.

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6
Q

Define an Ion?

A

An ion is an atom that has lost or gained an electron.

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7
Q

Write the electronic configuration (s,p) for a specific element.

A

(This would be specific to the element, e.g. for Oxygen: 1s² 2s² 2p⁴).

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8
Q

Define Isotopes?

A

Isotopes have the same atomic number but different mass numbers.

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9
Q

What are Allotropes?

A

Allotropes are different physical forms of the same element, differing in the way they are bonded.

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10
Q

Define Amphoteric?

A

An amphoteric substance can act as both an acid and a base.

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11
Q

Define Relative Atomic Mass?

A

Relative atomic mass is the average mass of an atom of an element compared to one twelfth the mass of C-12.

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12
Q

Define Electronegativity?

A

Electronegativity is the attraction that an atom has for a shared pair of electrons in a covalent bond.

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13
Q

Define Ionisation Energy?

A

Ionisation energy is the energy required to remove the most loosely bound electron from a neutral gaseous atom.

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14
Q

Why does atomic radii decrease across a period?

A

Atomic radii decrease across a period due to increasing nuclear charge.

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15
Q

Why does atomic radii increase down a group?

A

Atomic radii increase down a group due to increased shielding or screening.

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16
Q

Define Principle Quantum Number?

A

The principle quantum number indicates the main energy level of an electron.

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17
Q

Define Subsidiary Quantum Number?

A

The subsidiary quantum number gives the sublevel energy of an electron.

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18
Q

Define Magnetic Quantum Number?

A

The magnetic quantum number gives the direction of the orbital.

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19
Q

Define Spin Quantum Number?

A

The spin quantum number indicates the spin of the electron (+ or -).

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20
Q

Define Catalyst?

A

A catalyst alters the rate of a reaction without being used up.

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21
Q

Define Dipole Moment?

A

A dipole moment occurs when the centres of charge do not coincide, resulting in an asymmetrical distribution.

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22
Q

Define No Dipole Moment?

A

No dipole moment occurs when the centres of charge coincide, resulting in a symmetrical distribution.

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23
Q

Write the equation E2 - E1 = hf.

A

E2 is the energy at the higher energy level (excited state), E1 is the energy at the ground state, h is Planck’s constant, and f is the frequency of the photon.

24
Q

Define Transition Elements?

A

Transition elements have variable valency, are good catalysts, form coloured compounds, and have a partially filled d subshell.

25
Q

Define Strong Acid?

A

A strong acid is a good proton donor and is fully dissociated.

26
Q

Define Weak Acid?

A

A weak acid is a poor proton donor and is slightly dissociated.

27
Q

Define Strong Base?

A

A strong base is a proton acceptor.

28
Q

Define Weak Base?

A

A weak base is a poor proton acceptor.

29
Q

Define Conjugate Base?

A

A conjugate base is formed when a proton is removed.

30
Q

Define Conjugate Acid?

A

A conjugate acid is formed when a proton is added.

31
Q

Define pH?

A

pH is defined as -log₁₀[H⁺].

32
Q

Indicators used in acid-base titrations.

A

Methyl orange (for strong acid vs. weak base), Phenolphthalein (for weak acid vs. strong base).

33
Q

Example of an Acidic Oxide?

A

Carbon Dioxide.

34
Q

Example of an Amphoteric Acid?

A

Water.

35
Q

Define Electronegativity (again)?

A

Electronegativity is the relative measure of attraction for a shared pair of electrons in a covalent bond.

36
Q

Define Binary Compound?

A

A binary compound is made up of two elements.

37
Q

Types of Bonds?

A

Ionic, covalent, and polar covalent.

38
Q

Flame test: Potassium?

A

Purple/Lilac.

39
Q

Flame test: Sodium?

A

Yellow/Orange.

40
Q

Flame test: Lithium?

A

Red/Crimson.

41
Q

Flame test: Strontium?

A

Red.

42
Q

Flame test: Copper?

A

Green.

43
Q

Flame test: Barium?

A

Green.

44
Q

Why does sodium chloride conduct electricity in solution but not in a solid state?

A

Sodium chloride conducts electricity in solution because ions are free to move.

45
Q

Define Valency?

A

Valency is the number of electrons an atom of an element gives, takes, or shares when bonding.

46
Q

How to calculate the percentage element in a compound?

A

(Mass of element in the compound / Total mass of compound) x 100.

47
Q

Define Heat of Solution?

A

Heat of solution is the heat or energy involved when one mole of a substance is dissolved in excess water.

48
Q

Define Heat Change in a reaction?

A

Heat change refers to the energy change when the number of moles indicated in the balanced chemical equation reacts completely.

49
Q

Define Heat of Combustion?

A

Heat of combustion is the heat change when one mole of a substance is burned in excess oxygen.

50
Q

Define Heat of Formation?

A

Heat of formation is the heat change when one mole of a substance is formed from its elements in their standard state.

51
Q

Define Exothermic Reaction?

A

An exothermic reaction gives out heat or energy.

52
Q

Define Endothermic Reaction?

A

An endothermic reaction absorbs heat or energy.

53
Q

Shape of BF₃?

A

Triangular planar (120°).

54
Q

Shape of CO₂?

A

Linear (180°).

55
Q

Shape of H₂S?

A

V-shaped (104.5°).

56
Q

Shape of H₂O?

A

V-shaped (104.5°).

57
Q

Shape of CH₄?

A

Tetrahedral (109.5°).

physchem (10 decks)

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