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Gr 11 Physical Sciences > Chemistry Definitions > Flashcards

Chemistry Definitions Flashcards

1
Q

chemical bond

A

a mutual attraction between two atoms resulting from the
simultaneous attraction between their nuclei and the outer electrons.

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2
Q

Valence electrons

A

the electrons in the highest energy level of an atom in which there are electrons.

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3
Q

covalent bond

A

the sharing of electrons between two non-metal atoms to form a molecule.

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4
Q

molecule

A

A group of two or more atoms covalently bonded and that function as a unit.

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5
Q

bonding pair

A

a pair of electrons that is shared between two atoms in a covalent bond.

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6
Q

lone pair

A

a pair of electrons in the valence shell of an atom that is not shared with another atom.

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7
Q

electronegativity

A

a measure of the tendency of an atom in a molecule to attract bonding electrons.

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8
Q

non-polar covalent bond

A

a bond in which the electron density is shared equally between the two atoms.

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9
Q

polar covalent bond

A

a bond in which the electron density is shared unequally between the two atoms.

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10
Q

bond energy of a compound

A

the energy needed to break one mole of a substance’s molecules into separate atoms.

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11
Q

bond length

A

the average distance between the nuclei of two bonded atoms.

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12
Q

Mutually induced dipole forces or London forces:

A

Forces between non-polar
molecules

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13
Q

Dipole-dipole forces:

A

Forces between two polar molecules

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14
Q

Dipole-induced dipole forces:

A

Forces between polar and non-polar molecules

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15
Q

Hydrogen bonding:

A

Forces between molecules in which hydrogen is covalently bonded to nitrogen, oxygen or fluorine – a special case of dipole-dipole forces

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16
Q

Ion-dipole forces:

A

Forces between ions and polar molecules

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17
Q

Ion-induced dipole forces

A

forces between ions and non-polar molecules

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18
Q

Boiling point:

A

The temperature at which the vapour pressure of a substance equals atmospheric pressure.

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19
Q

Melting point:

A

The temperature at which the solid and liquid phases of a substance are at equilibrium.

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20
Q

Vapour pressure:

A

The pressure exerted by a vapour at equilibrium with its liquid in a closed system.

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21
Q

Solubility:

A

The property of a solid, liquid, or gaseous chemical substance (solute) to
dissolve in a solid, liquid, or gaseous solvent (solvent) to form a homogeneous solution.

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22
Q

Thermal expansion

A

the change in volume of a substance as the temperature increases.

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23
Q

thermal conductivity

A

the ability of a substance to conduct heat

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24
Q

surface tension

A

the force between particles on the surface of a liquid that tends to minimise the surface area of a liquid

25
Q

viscosity

A

a measure of how easily a liquid flows as particles move past each other

26
Q

capillarity

A

the tendency of a liquid to rise against gravity in a narrow tube

27
Q

specific heat

A

the amount of energy required to increase the temperature of a unit mass of a substance by 1 degree C

28
Q

(latent) heat of vaporisation

A

energy needed to change a given quantity of a substance into a gas

29
Q

Brownian motion

A

the random movement of particles in a liquid or gas caused by collisions between these particles and the motion of the liquid/gas.

30
Q

ideal gas

A

a gas with identical particles of zero volume with no IMFs all moving at the same speed

31
Q

real gas

A

gases that behave like ideal gases except at high pressures and/or low temperatures

32
Q

temperature

A

a measure of the average kinetic energy of a gas

33
Q

pressure

A

the force applied per unit area by a gas when the gas particles collide

34
Q

Boyle’s law:

A

The pressure of an enclosed gas is inversely proportional to the volume it occupies at constant temperature.

35
Q

Charles’ law:

A

The volume of an enclosed gas is directly proportional to its kelvin temperature provided the pressure is kept constant.

36
Q

Gay-Lussac’s Law

A

the pressure of a gas is directly proportional to its temperature in kelvin at
constant volume

37
Q

Avagadro’s Law

A

one mole of any gas occupies the same volume at the same
temperature and the same pressure

38
Q

one mole

A

the amount of substance having the same number of particles as
there are atoms in 12 g carbon-12.

39
Q

molar mass

A

the mass of one mole of a substance measured in g·mol-1

40
Q

concentration

A

the amount of solute per litre of solution.

41
Q

molecular formula

A

the total number of atoms of each element present in a molecule

42
Q

limiting reagent

A

a reagent that is completely used up in a chemical reaction

43
Q

heat of reaction (ΔH)

A

the energy absorbed or released per mole in a chemical reaction.

44
Q

exothermic reactions

A

reactions that release energy.

45
Q

endothermic reactions

A

chemical reaction that absorbs energy

46
Q

activation energy

A

the minimum energy needed for a reaction to take place.

47
Q

activated complex

A

the unstable transition state from reactants to products.

48
Q

Arrhenius theory:
Acids and Bases

A

An acid is a substance that produces hydrogen ions (H+)/hydronium ions (H3O+) when it dissolves in water.

A base is a substance that produces hydroxide ions (OH-) when it dissolves in water.

49
Q

Lowry-Brønsted theory:
Acid and Base

A

An acid is a proton/H+ ion donor.

A base is a proton/H+ ion
acceptor.

50
Q

Ampholyte

A

a substance that can act as either acid or base,

51
Q

acid-base indicator

A

a weak acid, or a weak base, which colour changes
as the H+ ion concentration or the OH- ion concentration in a solution changes.

52
Q

Redox reaction

A

a reaction involving an electron transfer. It always involves changes in oxidation numbers

53
Q

Oxidation:

A

A loss of electrons./An increase in oxidation number.

54
Q

Reduction:

A

A gain of electrons./A decrease in oxidation number.

55
Q

Reducing agent:

A

A substance that is oxidised/that loses electrons/whose oxidation
number increases.

56
Q

Oxidising agent:

A

A substance that is reduced/that gains electrons/whose oxidation
number decreases.

57
Q

synthesis reaction

A

a reaction in which 2 or more substances combine to form a new product

58
Q

decomposition reaction

A

a reaction in which a substance breaks up into two or more products

59
Q

displacement reaction

A

a reaction in which an ion of a less reactive element is replaced with an ion of a more reactive element.

Gr 11 Physical Sciences (5 decks)

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