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CHEM1111 > Bridging Course > Flashcards

Bridging Course Flashcards

(60 cards)

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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
The formula for the molecule of water is H2O. Is this an example of a diatomic or a triatomic molecule? Justify your answer.
It would be known as a **triatomic** molecule because there are 3 atoms in total that makeup the molecule.
26
The molecule of the element chlorine is written as Cl2. Why is this preferable as opposed to writing it as 2Cl?
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
Homogenous
**pure** compound
28
Electrolysis
the process of using electricity to **split** water into hydrogen and oxygen
29
mixtures are...
**hetero**genous
30
mass of a single atom
10^**-24** - 10^**-21** g
31
Proton
**1.673** × 10^**–24** g +1
32
Electron
0.0009 × proton mass = 0.0009 × 10^–24 g -1
33
Neutron
**1.675** × 10^**–24** g no charge
34
Nucleus
contains protons and neutrons
35
Alpha particle
**2 p**rotons and **2 n**eutrons joined together, very **strongly ionising**
36
Beta particle
*electron*, quite strongly **ionising**
37
Gamma
types of *electromagnetic radiation*, travels far in air, **weakly** ionising, **no charge**, **absorbed** in Earth's atmosphere
38
Ionising power
when radiation *collides* with atoms, it can cause the atoms to **lose electrons** and form **ions**
39
Positron
same mass as an electron, +1
40
Positron decay
when nucleus has to many protons it becomes unstable and needs to decay to **get rid** of excess *protons*
41
β+ particle
high speed electron
42
Avogadro's number
1 mole = **6.022** x 10^**23**
43
Nuclear decay
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
Nuclear force
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
Electron energy
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
atomic radius
the *larger* the atomic **number** of an atom, the more **electrons** it will have and the larger will be its atomic **radius**
47
Ground state
When all **electrons** in a given atom occupy the *lowest* possible energy **orbits**
48
Excited state
*one or more* **electrons** can jump to occupy a **higher** energy orbit for a brief period
49
Electromagnetic radiation
energy released by **excited electrons** *returning* to lower energy orbits The pattern of lines observed is the **atomic emission spectrum**
50
1st orbit level
can only hold **2 electrons**
51
2nd orbit level
can hold **8 electrons**
52
Noble gases are referred to as inert because...
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
Ion
When an *atom* acquires a **charge** and is no longer electrically neutral
54
Cation
ions which have a positive charge
55
Anion
ion has a negative charge
56
ide
*suffix* added to the name of the element to show that it is in a form an **anion**
57
isoelectronic
When atoms of *different* elements attain the **same electron arrangement** by forming **cations** or **anions**
58
metals form...
**cat**ions
59
non-metals form...
**an**ions
60
is ionisation energy spontaneous?
**No**, formation of cations from metal atoms requires this *energy* input

CHEM1111 (15 decks)

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