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Chemistry ALevel > Definitions - Module 2 > Flashcards

Definitions - Module 2 Flashcards

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1
Q

Atomic number

A

The number of protond/electons in an atom

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2
Q

Isotope

A

Atoms of the same element with different numbers of neutrons and masses

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3
Q

Mass number

A

number of protons + number of neutrons

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4
Q

Relative atomic mass

A

The weighted mean mass of an element relative to 1/12th the mass of an atom of Carbon-12

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5
Q

Relative isotopic mass

A

The mass of an isotope relative to 1/12th the mass of an atom of Carbon-12

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6
Q

Ion

A

Is a charged atom

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7
Q

Cation

A

Positive ion (fewer electrons than protons)

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8
Q

Anion

A

Negative ion (more electrons than protons)

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9
Q

Aqueous

A

Dissolved in water

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10
Q

1 mole

A

the amount of substance that contains Avogadro constant (6.02x10^23) particles

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11
Q

Avogadro constant

A

6.02x10^23mol^-1

The number of partilces in each mole of carbon-12

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12
Q

Molar mass

A

mass in grams in each mole of the substane (gmol^-1)

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13
Q

Molecular formulae

A

the number of atoms of each element in a molecule

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14
Q

Empirical formulae

A

the simplest whole number ration of atoms of each element in a compound

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15
Q

Relative formula mass

A

compares the mass of a formula unit with the mass of an atom of carbon-12

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16
Q

Relative molecular mass

A

compares the mass of a molecule with the mass of an atom of carbon-12

17
Q

Assumptions of the ideal gas equation

A

1) random motion
2) elastic collisions
3) negligible size
4) no intermolecular forces

18
Q

Stoichiometry

A

the ration of the amount in moles of each substance in a balanced symbol equation

19
Q

Percentage yield

A

actual yield/predicted yield x100

20
Q

Limiting reagent

A

The reactant that isnt in excess and will be completely used up first causing the reaction to stop

21
Q

Atom economy

A

Mr of desired products/Mr of all products x100

22
Q

A strong acid

A

completely ionises in water (releases all of it H+ ions)

23
Q

A weak acid

A

Partially ionises in water (releases a small proportion of its available H+ ions)

24
Q

Titrations can be used for

A

1) finding the concentraion of a solution
2) Identifying unknown chemicals
3) finding the purity og a substance

25
Q

REDOX rections

A

Involve both reduction and oxidation

26
Q

Atomic orbital

A

a region around the nucleus that cano hold up to 2 electrons. (SPDF)

27
Q

Ionic bonding

mainly metal and non-metal

A
  • electrostatic attraction between positive and negative ions
  • TRANSFER of electrons
28
Q

Covlent bonding (nonmetals)

A

strong electrostatic attraction between a SHARED pair of electrons and the nuclei of the bonded atoms

29
Q

A dative covalent/coordinate bond

A

a covalent bond in which the shared pair of elecrtons has been supplied by only 1 of the atoms

30
Q

Level of repulsion

A

bonded-pair/bonded-pair < bonded-pair/lone-pair < lone-pair/lone-pair
INCREASING

31
Q

Electronegativity

A

the attraction of a bonded atom for the pair of electrons

Most en: N,O,F,Cl
Least en: Li,Na,K

32
Q

Non-polar bond

A

the bonded electron pair is shared equally between the bonded atoms (atoms are the same or of similar electronegativity)

33
Q

Polar bond

A

The bonded pair of electrons is shared unequally between the bonded atoms.

34
Q

Dipole

A

Separation of opposite charges

35
Q

Types of intermolecular forces

A

1) London forces
2) Permanent dipole-dipole
3) Hyrdogen bonding

36
Q

London forces

A
  • exist in all molecules

- more electrons=stronger

37
Q

Permanent dipole-dipole

A

-Between different molecule with permanent dipoles

38
Q

Hyrdogen bonds

A

-permanent dipole-dipole between a hydrogen atom attached to (O,N,F) and an elecytronegative atom with a lone pair of electrons

39
Q

Why is Ice less dense than water?

A

-Hydrogen bonds hold water molecules apart in open lattice structures (molecules further apart than in watert)

Chemistry ALevel (5 decks)

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