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CHEM1110 > Week 2 > Flashcards

Week 2 Flashcards

1
Q

Atomic Mass

A

A relative comparison system using the carbon-12 isotope to assign a relative mass value to atoms

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2
Q

Who assigned atomic mass?

A

Dalton

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3
Q

How many atomic mass units does carbon-12 have?

A

12u (or Da)

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4
Q

1 atomic mass unit =

A

1/2 mass of the carbon-12 isotope

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5
Q

1 amu in grams =

A

1.67 x 10*-24g

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6
Q

Define percentage composition

A

Describes the quantities of elements or compounds that comprise a body of matter. Based on percentage by mass.

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7
Q

% composition formula

A

% composition =

(mass of component/total mass of the whole) x 100

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8
Q

Average atomic mass composition %

A

sum of:

(% composition/100) x atomic mass of each isotope

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9
Q

Stoichiometry

A

The ratio of chemicals in a substance

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10
Q

Define mole

A

a unit used to relate the atomic mass units to gram quantity masses. It is the number of atoms in a gram equivalent to 6.022 x 10*23 atoms (based on atomic or molecular mass)

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11
Q

Avogardo’s number

A

mass in grams numerically equal to an element’s atomic mass that contains 6.02 x 10*23 atoms

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12
Q

Number of particles =

A

number of moles x avogardo’s number

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13
Q

how is Avogardo’s number derived?

A

equal to the number of atoms present in 12 grams of carbon-12

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14
Q

Define molar mass (element)

A

Mass in grams numerically equivalent to the atomic mass (mass number)

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15
Q

Define molar mass (compound)

A

Mass in grams numerically equivalent to the formula mass (add up the atomic masses of the elements in the compound)

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16
Q

Equation to find # moles in a substance

A

mass of substance/molecular mass

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17
Q

Elements that can be found naturally in their elemental atomic states

A
  • non-reactive metals
  • inert (noble) gases
  • oxygen and nitrogen
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18
Q

Define compounds

A

when elements exist in definite combinations with one or more atoms by sharing electrons

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19
Q

Are compounds man-made or natural?

A

Both

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20
Q

Types of compounds

A
  • molecules (discrete)
  • ionic compounds (infinite lattice)
  • covalent bonds (infinite lattice)
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21
Q

What are molecules

A
  • compound with at least two atoms
  • held together by chemical forces
  • smallest representative unit of a pure substance
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22
Q

types of molecules

A
  • monatomic
  • diatomic
  • polyatomic
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23
Q

monatomic molecules

A
  • molecule made up of one type of atom
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24
Q

diatomic molecules

A
  • molecule made up of 2 types of atoms
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25
Q

polyatomic molecules

A
  • molecule made up of more than 2 types of atoms

- make up the vast majority of molecules

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26
Q

molecular formula

A

shows the exact number of atoms in each element (e.g. h2o). Doesn’t show how atoms are arranged

27
Q

Structural formula

A
  • shows how atoms are arranged - connectivity of atoms
28
Q

Ion

A

Charged atoms that occur when theres an imbalance in the number of protons and electrons present. Forms from loss or gain of electrons and occur without alteration of nucleus.

29
Q

Cation vs anion

A

cations: lost electrons (more positive) - mainly metallic
Anions: gained one or more electrons (more negative) - mainly non-metallic

30
Q

polyvalent ions

A

Ions that can adopt more than one charged state, mostly coming from the transition series of the periodic table

31
Q

Common polyvalent ions

A
  • Cr (2+ and 3+)
  • Mn (2+, 3+, 4+, 7+)
  • Fe (2+ and 3+)
  • Cu (+ and 2+)
  • Co (2+ and 3+)
32
Q

What are ionic compounds

A

Compounds formed when you combine something that has lost an electron with something that has gained an electron.

33
Q

Ionic compound properties

A
  • contain sufficient cations and anions to maintain electrical neutrality
  • crystalline solids
  • conduct electricity in molten state
  • high melting points
34
Q

Ionic liquids

A
  • ionic substances that are liquid at room temperature. They are comprised of an organic cation and polyatomic anion
35
Q

Ionic solids structure

A
  • three dimensional lattice

- do not contain discreet molecular units; only a repeating unit cell

36
Q

Binary compounds

A

Compounds that contain only 2 elements. Can be ionic or covalent

37
Q

Binary ionic compounds

A
  • salts
  • metal and non-metal
  • electrons are transferred
  • always involve a cation and an anion
38
Q

Binary covalent compounds

A
  • two non-metals

- electrons are shared

39
Q

Naming rules for binary covalent compounds

A
  1. first element in the name (most metallic) named in full
  2. remaining element named as if it was an anion (-ide)
  3. mono, di, tri etc. prefixes used to indicate the number of atoms of the same type that are present
  4. -ide used to indicate binary formation
  5. prefix mono may be dropped for first element
40
Q

Location of more metallic elements in periodic table

A
  • further left hand side or bottom of periodic table
41
Q

Naming polyvalent compounds

A
  • naming always has to include what the charge is
42
Q

Polyvalent compounds

A

Ionic compounds that can adopt more than one charge

43
Q

Naming anions

A

Add the suffix -ide to the parent atom

44
Q

Cation

A

Name stays the same as the parent atom

45
Q

Chemical formulae parts

A
  • most metallic element first, non-metallic element second
  • number of atoms present (shows the ratio)
  • chemical formula must have a net charge of zero
46
Q

Empirical formula

A

Formula of a compound that presents constituent elements as whole number ratios (simplify the molecular formula)

47
Q

When is the empirical formula most used?

A

When naming ionic compounds

48
Q

How to find an empirical formula based on molar mass

A
  • Assume 100g mass (because its a percentage) and assign values to constituent elements accordingly
  • divide mass by molecular weight to find out how many moles there are
  • normalise by dividing by smallest number
49
Q

Polyatomic ions

A

Possesses the ability to gain or lose electrons

50
Q

Carbonate (polyatomic ion)

A

(CO3)^2

51
Q

Permanganate

A

(MnO4)^-

52
Q

Nitrate

A

(NO3)^-

53
Q

Nitrite

A

(NO2)^-

54
Q

Sulphate

A

(SO4)^2-

55
Q

Sulphite

A

(SO3)^2-

56
Q

Hydroxide

A

HO^-

57
Q

Halogens

A

Inorganic acids found in the 2nd last column of the periodic table that combine with hydrogen (covalent bond) to form binary gases. When dissolved in water these gases form acidic solutions

58
Q

Binary gases

A

Any gas made of two gaseous components mixed with each other

59
Q

Oxo-Acids

A

Acidic substances formed with carbon, nitrogen, phosphorus and sulphur in combination with oxygen and hydrogen

60
Q

Acid

A

Anything that can donate a hydrogen atom

61
Q

Common oxo-acids

A
  • carbonic acids
  • phosphoric acid
  • nitric acid
  • sulphuric acid
62
Q

What does the charge of polyoxo anions indicate?

A
  • the number of protons (H) that can combine to form the corresponding acid
63
Q

What are hydrates?

A

Compounds that have a specific number of water molecules trapped in ionic lattices. It doesn’t affect the chemistry but must be included in calculations relating to mass.

64
Q

Naming of hydrates

A

salt name + greek prefix (e.g. di, hexa etc) - ‘hydrate’

CHEM1110 (5 decks)

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