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Chemistry IB SL 42S > Chemistry IB SL Exam: Paper 1 and 2 > Flashcards

Chemistry IB SL Exam: Paper 1 and 2 Flashcards

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1
Q

Define Convergence

A

In each series, the lines converge meaning higher levels/shells get closer together

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2
Q

Define Emission Spectra

A

Refers to when electrons are excited to a higher energy level, then return to a lower energy level, they release a photon of specific energy, as shown by a specific frequency of light

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3
Q

Isotope of uranium is used for?

A

Nuclear power

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4
Q

¹³¹I or ¹²⁵I is used for?

A

Medical tracers

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5
Q

⁶⁰Co is used for?

A

Radiotherapy

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6
Q

Which of the following increase the amount of product in electrolysis?
I. Increasing the charge of the ion
II. Increasing the current
III. Increasing the duration

A

II and III

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7
Q

Reducing agent 2

A

— reduces other species and, in the process, is itself oxidized

— gives electrons to something

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8
Q

Oxidizing agent2

A
  • – oxidizes other species and, in the process, is itself reduced
  • – takes electron away from something
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9
Q

Oxidation Number 2

A

— A purely formal concept that regards all compounds as ionic and assigns charges to the components accordingly

— it provides a guide to the distribution of electrons

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10
Q

REDOX reaction2

A

— A reaction that includes both oxidation and reduction

— If something is oxidized and something is reduced in a reaction, it is a REDOX reaction

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11
Q

Reduction 2

A

— gain of electron

— Decrease in oxidation number

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12
Q

Oxidation 2

A

— loss of electrons

    --- increase in oxidation number
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13
Q

How much does 1 mole of gas occupy at standard temperature and pressure?

A

22.7 L/mol

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14
Q

Molecular Formula

A

The actual number of atoms of different elements covalently bonded in a molecule

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15
Q

Empirical Formula

A

The simplest whole number ratio of atoms of different elements in a compound

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16
Q

Nucleophile

A

Reagents that have a non-bonding pair of electrons; attracted to the C atom in the halogenoalkanes during substitution reactions

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17
Q

saturated

A

containing no C=C double bonds

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18
Q

unsaturated

A

containing at least one C=C double bond

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19
Q

Period

A

horizontal row of elements in the Periodic table

within a period the atoms of the elements have the same number of shells but with an increasing number of electrons in the outer shell

20
Q

Group

A

vertical column of elements in the Periodic table

the atoms of the elements in the same group all have the same outer shell structure but an increasing number of inner shells.

21
Q

What is the geometry of water?

A

Tetrahedral

22
Q

Oxidising agent

A

accepts electrons and becomes reduced

23
Q

Reducing agent

A

donates electrons and becomes oxidised

24
Q

Solute

A

the substance dissolved in a solvent forming a solution

25
Q

Solvent

A

the liquid that dissolves another substance or substances to form a solution

26
Q

Solution

A

a homogeneous mixture of a liquid (solvent) with another substance (solute)

there is usually some interaction between the solvent and solute molecules

27
Q

Concentration

A

the amount of solute in a known volume of solution

expressed as dm^-3

28
Q

Continuous Spectrum

A

shows an unbroken sequence of frequencies

eg. the spectrum of visible light

29
Q

Line Spectrum

A

an emission spectrum that has only certain frequencies of light.

produced by excited atoms and ions as they fall back to a lower energy level

30
Q

Heterogeneous

A

Have different properties

31
Q

Mass number

A

sum of an atom’s protons & neutrons

32
Q

Isotopes of an element

A

atoms of the same element (same atomic number /Z) with a different number of neutrons (different mass number /A)

33
Q

First ionisation energy

A

the minimum energy required to remove a mole of electrons from a mole of gaseous atoms to form a mole of univalent cations in the gaseous state

it is the enthalpy change for the reaction : X(g) → X^+ + e^-

34
Q

Electronegativity

A

measure of the tendency of an atom in a moloecule to attract a shared pair of electrons towards itself

35
Q

Endothermic reaction 3

A

Reaction in which energy is absorbed from surroundings

Enthalpy change = +ve

Forms products with weaker bonds than the reactants

36
Q

Exothermic reaction 3

A

Reaction that releases heat to surroundings

Enthalpy change = -ve

Forms products with stronger bonds than the reactants

37
Q

Average bond enthalpy 2

A

the energy required to break 1 mole of covalent bonds in the reactant, all reactants and products being in the gaseous state.

It is an average value because it takes into account the different energies in a bond between the same atoms in different molecules

38
Q

Standard state 5

A

standard state of an element is its most stable state under the specified conditions

A precisely defined reference state as:

- Temperature of a substance at exactly 298K
- Pressure of gaseous substance are exactly 1 atm
- liquids & solids are pure - aqueous solutions are exactly 1 mol per dm cubed
39
Q

Modifying the side chain in penicillin will make them stronger or weaker against penicillinase enzyme?

A

Stronger, makes them more resistant

40
Q

Meningitis and gonorrhea can be treated with what drug?

A

Penicillin G

41
Q

A tertiary amine had N joined to _____ C atoms

A

3 (3 alkyl groups)

42
Q

Which is a more potent analgesic? Diamorphine or morphine? Why?

A

Diamorphine is a more potent analgesic than morphine because it is better at crossing the blood brain barrier

43
Q

Define Law in science

A

A description of regular patterns of behavior

44
Q

Define Theory in science

A

An explanation that provides an understanding across a range of phenomena and disciplines

45
Q

Define atom

A

Smallest part of an element

46
Q

Define Compound

A

2 or more elements chemically bonded to each other

47
Q

Homogeneous

A

Have uniform property

Chemistry IB SL 42S (6 decks)

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