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CHEM1111 > Bridging Course > Flashcards

Bridging Course Flashcards

1
Q

Alkali Metals (+1)

A

Lithium (Li)
Sodium (Na)
Potassium (K)
Rubidium (Rb)
Caesium (Cs)

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2
Q

Alkali Earth Metals (+2)
first group

A

Beryllium (Be)
Magnesium (Mg)
Calcium (Ca)
Strontium (Sr)
Barium (Ba)

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3
Q

Alkali Earth Metals (+2)
second group

A

Boron (B) (+3)
Aluminium (Al)
Gallium (Ga)
Indium (In)
Thallium (Tl)

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4
Q

Alkali Earth Metals (+2)
third group

A

Carbon (C) (+4)
Silicon (Si)
Germanium (Ge)
Tin (Sn)
Lead (Pb)

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5
Q

Alkali Earth Metals (+2)
fourth group

A

Nitrogen (N) (+5)
Phosphorus (P)
Arsenic (As)
Antimony (Sb)
Bismuth (Bi)

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6
Q

Alkali Earth Metals (+2)
fifth group

A

Oxygen (O)
Sulphur (S)
Selenium (Se)
Tellurium (Te)

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7
Q

Halogens (-1)

A

Fluorine (Fl)
Chlorine (Cl)
Bromine (Br)
Iodine (I)

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8
Q

Noble gases (-2)

A

are naturally monatomic
Helium (He)
Neon (Ne)
Argon (Ar)
Krypton (Kr)
Xenon (Xe)
Radon (Rn)

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9
Q

Some transition metals (-3)

A

Chromium (Cr)
Manganese (Mn)
Iron (Fe)
Nickel (Ni)
Copper (Cu)
Zinc (Zn)
Silver (Ag)
Cadmium (Cd)
Platinum (Pt)
Gold (Au)
Mercury (Hg).

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10
Q

Element

A

substance which cannot be broken down into simpler component substances

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11
Q

Metals (physical)

A

Shiny when freshly cut
Conduct heat and electricity well
Malleable
Ductile

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12
Q

Non-metals (physical)

A

Powders or gases
Do not conduct well
Solids will be brittle

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13
Q

Chemical change

A

whenever a chemical bond is broken or formed

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14
Q

Physical change

A

when mixtures are separated into their pure components by physical methods such as filtration, distillation or even by making use of the different densities of components

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15
Q

Mixture

A

consists of different elements or compounds which have been physically mixed together (e.g. rocks and sand)
inherently impure

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16
Q

Compound

A

A combination of substances. At least two or more different types of atoms are joined together by chemical bonds

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17
Q

Atom

A

smallest possible unit of an element. Each elements atoms are unique to each element

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18
Q

Molecule

A

atoms bonded together (e.g. CO2)

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19
Q

Allotrope

A

the various forms in which an element may occur. An element may occur with more than one arrangement of its constituent atoms.

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20
Q

Monatomic

A

contain one atom

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21
Q

Diatomic

A

contain 2 atoms

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22
Q

Triatomic

A

contain 3 atoms

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23
Q

In what fundamental way do compounds differ from elements?

A

Elements are naturally occurring substances and cannot be reduced to a simpler form, whereas compounds are a combination of these substances with at least 2 different types of atoms that are chemically bonded

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24
Q

Can one write a formula for air? Explain why.

A

No because it is a mixture of elements (oxygen, nitrogen and argon) and compounds (carbon dioxide and water vapour) and this mixture will vary depending on samples so there is no set formula

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25
Q

The formula for the molecule of water is H2O. Is this an example of a diatomic or a triatomic molecule? Justify your answer.

A

It would be known as a triatomic molecule because there are 3 atoms in total that makeup the molecule.

26
Q

The molecule of the element chlorine is written as Cl2. Why is this preferable as opposed to writing it as 2Cl?

A

This is because Cl2 exists as diatomic in nature and by saying 2Cl you would be saying that there is two chlorine atoms that are NOT chemically bonded

27
Q

Homogenous

A

pure compound

28
Q

Electrolysis

A

the process of using electricity to split water into hydrogen and oxygen

29
Q

mixtures are…

A

heterogenous

30
Q

mass of a single atom

A

10^-24 - 10^-21 g

31
Q

Proton

A

1.673 × 10^–24 g
+1

32
Q

Electron

A

0.0009 × proton mass = 0.0009 × 10^–24 g
-1

33
Q

Neutron

A

1.675 × 10^–24 g
no charge

34
Q

Nucleus

A

contains protons and neutrons

35
Q

Alpha particle

A

2 protons and 2 neutrons joined together, very strongly ionising

36
Q

Beta particle

A

electron, quite strongly ionising

37
Q

Gamma

A

types of electromagnetic radiation, travels far in air, weakly ionising, no charge, absorbed in Earth’s atmosphere

38
Q

Ionising power

A

when radiation collides with atoms, it can cause the atoms to lose electrons and form ions

39
Q

Positron

A

same mass as an electron, +1

40
Q

Positron decay

A

when nucleus has to many protons it becomes unstable and needs to decay to get rid of excess protons

41
Q

β+ particle

A

high speed electron

42
Q

Avogadro’s number

A

1 mole = 6.022 x 10^23

43
Q

Nuclear decay

A

When an isotope has significantly more or less neutrons than the number of protons in its nucleus, it is usually unstable and undergoes a nuclear spontaneously over a period of time - radioactive species

44
Q

Nuclear force

A

operating between protons, between neutrons and between protons and neutrons is the reason why the nucleus is stable provided there is an appropriate ratio of protons to neutrons.

It is a nuclear force and is not experienced by electrons.

45
Q

Electron energy

A

Electrons occupying orbits closest to the nucleus have the lowest energy while electrons in orbits further out from the nucleus have higher energy.

This is because, in order to overcome electrostatic attraction to the nucleus, energy must be supplied to an electron to move it from an orbit closer to the nucleus to an orbit further out

46
Q

atomic radius

A

the larger the atomic number of an atom, the more electrons it will have and the larger will be its atomic radius

47
Q

Ground state

A

When all electrons in a given atom occupy the lowest possible energy orbits

48
Q

Excited state

A

one or more electrons can jump to occupy a higher energy orbit for a brief period

49
Q

Electromagnetic radiation

A

energy released by excited electrons returning to lower energy orbits

The pattern of lines observed is the atomic emission spectrum

50
Q

1st orbit level

A

can only hold 2 electrons

51
Q

2nd orbit level

A

can hold 8 electrons

52
Q

Noble gases are referred to as inert because…

A

they do not normally enter into any chemical reactions

atoms of noble gases require too much energy to be involved in any redistribution of electrons with other atoms

53
Q

Ion

A

When an atom acquires a charge and is no longer electrically neutral

54
Q

Cation

A

ions which have a positive charge

55
Q

Anion

A

ion has a negative charge

56
Q

ide

A

suffix added to the name of the element to show that it is in a form an anion

57
Q

isoelectronic

A

When atoms of different elements attain the same electron arrangement by forming cations or anions

58
Q

metals form…

A

cations

59
Q

non-metals form…

A

anions

60
Q

is ionisation energy spontaneous?

A

No, formation of cations from metal atoms requires this energy input

CHEM1111 (15 decks)

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