Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

LC Chemistry > Mix > Flashcards

Mix Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
0
Q

Chemical equilibrium is said to be dynamic because…

A

At equilibrium there are reactions continually occurring and the rate of the forward reaction equals the rate of the reverse reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
1
Q

Reversible reaction

A

Takes place in either direction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Balanced equation for the formation of ammonia

A

N2 +3H2 —-> 2NH3

<—-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Le chatelier’s principle

A

When a system at equilibrium is subjected to a stress, the equilibrium shifts in such a way as to minimise the effect of the stress

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Equation for the reversible reaction between cobalt chloride and water

A

CoCl4 -2 + 6H2O –> Co(H2O) +
<–
4Cl-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

The contact process

A

Process used to make sulfur trioxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

The Haber process

A

Process used to make ammonia

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Rate of a chemical reaction

A

The change on concentration in unit time if any one reactant or product

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Catalyst

A

A substance that alters the rate of a reaction but is chemically unchanged at the end of the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Energy Level

A

A region of definite energy within an atom that electrons can occupy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Line Spectrum

A

A series of coloured lines against a dark background

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

The emission spectrum of an element

A

is characteristic of that element, and is different from that of any other element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

The absorption spectrum of an element

A

The spectrum observed after white light has been passed through the element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

The Heisenberg Uncertainty Principle

A

States that it is not possible to determine at the same time the exact position and velocity of an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

An Atomic Orbital

A

A region in space where there is a high probability of finding an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

The Aufbau Principle

A

States that electrons will occupy the lowest energy level available

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

An Energy Sub-level

A

A group of atomic orbitals within an atom all of which have the same energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Potassium electron confirguration? How many

(i) energy levels (ii) energy sub-levels
(iii) individual orbitals

A 
1s2
2s2 2p6 
3s2 3p6
4s1  
Energy levels = 3 energy sublevels = 6 Orbitals = 10
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Which is the energy level, energy sublevel and atomic orbital?
3px2

A

Energy level is the number in front (3)
Energy sub-level is the part of the letter
(X)
Atomic orbital is the entire letter group
(P group)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Ionisation Energy

A

A measure of the amount of energy needed to remove electrons from atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

The First Ionisation Energy

A

The energy required to remove the most loosely bound electron from one mole of gaseous atoms in its ground state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

The Second Ionisation Energy

A

The energy required to remove the most loosely bound electron from each singly charged positive ion in a mole of these ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

The Atomic Radius of an element

A

Half the distance between the nuclei of two atoms of the element that are joined together by a single covalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Factors that affect the size of the atomic radius

A

Nuclear charge, number of energy levels and the screening effect of the inner electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

In a periodic table, does the atomic radius increase or decrease on going left to right across a period?

A

Decrease

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

In a periodic table, does the atomic radius increase or decrease on going down a group?

A

Increase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

The first ionisation energy values increase going across a period because?

A

Of the increase in nuclear charge and the decrease in atomic radius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

The first ionisation values decrease going down a group because?

A

Of the increase on atomic radius and the screening effect of the inner energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Bohr’s theory of the hydrogen atom

A

The hydrogen electron is restricted to those regions of the atom that have certain energy values (energy levels)

38
Q

Louis de Broglie stated that…

A

Electrons, like light, have the properties of waves as well as of particles

39
Q

Water Crystallisation

A

Substances that contain molecules of water in definite proportions locked into a crystal structure

40
Q

Standard solution

A

One whose concentration is accurately known

41
Q

Primary standard

A

A substance used to make a standard solution direct/ very pure and stable

42
Q

Primary standard example..

A

Anhydrous sodium carbonate

43
Q

Percentage Yield

A

Actual Yield
————–✖️100
Theoritcal Yield

44
Q

A Bronsten/Lowery acid

A

A proton donor

45
Q

A Bronsten/Lowery base

A

Proton acceptor

46
Q

Arrhenius’ definition of an acid

A

Dissociates in water in to produce H+

47
Q

Arrhenius’ definition of a base

A

Dissociates in water to produce OH-

48
Q

A conjugate pair

A

Consists of an acid and a base that differ by one proton

49
Q

The shortcomings of Arrhenius’ theory

A

1) . Hydronium ions (H3O+) are formed, not H+

2) . Restricted to reactions in water

50
Q

aA + bB —-\ cC + dD
-—
What is Kc? (equilibrium constant)

A

Kc = {C}c {D}d
———–
{A}a {B}b

51
Q

If Kc is < 1 …

A

The concentration of the products is less than the reactants

52
Q

Factors that effect rate of reaction

A 
Catalysts (speeds up reaction), concentration (more particles bump into each other more frequently), temperature (particles more energised), 
surface area (increase surface area for reaction)
53
Q

The rate of a chemical reaction is

A

The change in concentration in unit time of any one reactant or product

54
Q

The instantaneous rate of reaction

A

Is the rate at a particular point int time during a reaction

55
Q

A heterogeneous catalyst

A

Is a catalyst in a different phase to the reactants

56
Q

A homogenous catalyst

A

Is in the same phase the reactants

57
Q

Autocatalysis

A

Occurs when a product of a reaction increases the rate of the reaction

58
Q

Activation energy

A

Is the minimum energy with which particles need to collide to cause a reaction

59
Q

What is the influence of temperature on reaction rate?

A

The higher the temp., the greater the molecules have and the greater their average speed. This has two effects:

(a) the number of collisions per second is increased
(b) each collision is more energetic and a higher amount of collisions have the necessary activation energy for reaction to occur

60
Q

Radioactivity

A

Is defined as the spontaneous breaking up of unstable nuclei accompanied by the emission of radiation

61
Q

Alpha particles are

A

Helium nuclei with a positive charge and little penetrating ability

62
Q

Beta particles are

A

Electrons with a negative charge and greater penetrating ability than alpha

63
Q

Gamma rays are

A

high energy electromagnetic radiation with power penetrating ability

64
Q

Difference between nuclear and chemical reactions?

A

Nuclear reactions :
➡️ new element may be formed
➡️ changes occur in the nucleus
➡️ no chemical bonds broken or formed

65
Q

The half-life of a radioactive isotope

A

Is the time taken for half of the atoms in a sample of the isotope to decay

66
Q

Electroplating

A

Is the coating of metal into the surface of another metal using electrolysis

67
Q

The valency of an element is

A

The Humber of bonds each atom of the element forms when it reacts

68
Q

A covalent bond is

A

Formed when two atoms share a pair if electrons

69
Q

A sigma bond

A

Is a covalent bond between two atoms formed by end- on overlapping of orbitals

70
Q

A pi bond

A

Is a covalent bond between two atoms formed by sideways overlapping of orbitals

71
Q

A polar covalent bond

A

Is a covalent bond in which there is unequal sharing of electrons

72
Q

Electronegativity

A

The relative attraction of an atom for shared pairs of electrons in a covalent bond

73
Q

Methyl orange (i) pH (ii) colour in acid (iii) colour in base

A

(i) 3-5 (ii) red (iii) yellow

74
Q

Litmus (i) pH (ii) colour in acid (iii) colour in base

A

(i) 5-8 (ii) red (iii) blue

75
Q

Phenolphthalein (i) pH (ii) colour in acid (iii) colour in base

A

(i) 8-10 (ii) colourless (iii) pink

76
Q

The biochemical oxygen demand

A

The amount of dissolved oxygen in ppm used up by a sample over a period of five days in the dark

77
Q

If the forward reaction is exothermic the Kc …

A

Decreases as the temp rises

78
Q

If the forward reaction is endothermic the Kc …

A

Increases as the temp rises

79
Q

The electron pair repulsion theory

A
  • The electron pairs in the outer shell of the central atom repel each other and end up as far apart as geometrically possible
  • Lone pairs have a greater repelling power than bond pairs
80
Q

The oxidation number

A

The charge that the atom appears to have when the electrons are distributed according to certain rules

LC Chemistry (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions