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Chemistry Flashcards

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1
Q

What are the 3 Subatomic Particles?

A

Protons - Positive Charge
Neutrons - Neutral Charge
Electrons - Negative Charge

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2
Q

What is the Atomic Number?

A

The atomic number of an element is the number of protons in the nucleus of the atom.

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3
Q

What is the Mass Number?

A

The mass number of an element is the total number of protons and neutrons (nucleus) in the atom.

Protons and neutrons have approximately the same mass but electrons mass is negligible

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4
Q

What are Neutral Atoms?

A

An atom represented on the Periodic table has an
overall neutral charge.
• Number of protons (+) = number of electrons (-)

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5
Q

What are Electron Shells?

A

Electrons may be visualised as moving within a
region of space surrounding the nucleus
labelled
K,L,M,N or 1,2,3,4.

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6
Q

What is the Electron Configuration?

A

K = Max 2 Electrons
L = Max 8 Electrons
M = Max 18 Electrons (8 for the first 20 Elements)
N = Max 32 Electrons (2 for the first 20 Elements)

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7
Q

What is the Ground State?

A

Electrons “prefer” to be at the lowest energy level to be most stable.
Electrons fill the lowest energy shells first, to be in the ground state.

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8
Q

What is Mendeleev’s table?

A

Mendeleev organised the elements according to similar chemical properties and in order of their atomic mass.

He left gaps for elements that he predicted existed but hadn’t been discovered yet.

He did this by looking at the properties of the
elements above and below and “averaging”

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9
Q

What are the ‘Groups’ of the periodic table?

A
  • Vertical Columns
  • Numbered 1-18
    Properties -
    • Have similar chemical properties
    • React in similar ways
    • Same number of valence electrons
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10
Q

What are the ‘Periods’ of the periodic table?

A
  • Horizontal Rows
  • Numbered 1-7
    Properties -
    • Properties will increase or decrease across the period
    • Same number of electron shells
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11
Q

What is the correlation between groups, periods and electron shells?

A

• All elements in the same group have the same number of valence (outer-shell) electrons
• All elements in the same period have the same number of electron shells

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12
Q

What are the properties of metals?

A

• are shiny
• have high melting and boiling points
• are good conductors of heat and electricity
• are ductile - can be drawn into long, thin wires
• are malleable - can be beaten into shapes

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13
Q

Transition Metals?

A

• Metals in the middle of the periodic table
• Usually hard and dense
• Often exist in multiple forms
o Iron: Fe2+ and Fe3+

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14
Q

Lanthanides and Actinides?

A

• Fit into the periodic table next to the transition metals
• Most are synthetic elements with some exceptions (U)
• Many are radioactive and/or unstable

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15
Q

Non-metal properties?

A

• are dull
• are brittle - they will shatter when bent
• have low melting and boiling points
• are poor conductors of heat and electricity

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16
Q

Metalloids?

A

• 7 elements between the metals and the non-metals
• Have some properties of metals - shiny
• And some properties of non-metals - brittle
• Semi-conductors - good conductivity between conductors and insulators

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17
Q

Metals?

A

• More than 80% of the elements (91 out of 118)
• Important to development of human society
• Diverse properties make them very useful

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18
Q

Metals on the periodic table?

A

Alkali metals (Group 1)
Alkaline earth metals (Group 2)
Transition metals (Groups 3– 12)
Post-transition metals
Lanthanides
Actinides

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19
Q

Alkali Metals?

A

Highly reactive with air and water
Reactivity increases down the group
Soft –> cut with a knife
Dull on the outside, but shiny on the
inside because they have an oxide
layer
Lower density than water –> float

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20
Q

Alkaline Earth Metals?

A

Highly reactive (less so than
Group 1)
Reactivity increases down the
group
Shiny and silvery white.
Low melting and boiling points.

21
Q

Metallic Bonding?

A

Single atoms of metals don’t exist.They exist in large lattices of atoms that are
joined together by chemical bondsThese chemical bonds are called metallic bonds.

22
Q

What happens to electrons in metallic bonding?

A

Electrons become delocalised

23
Q

How does metallic bonding explain properties of metals?

A

Shiny because the delocalised electrons reflect light
High melting and boiling points because the metallic bonds are very
strong, so it takes a lot of energy to break them
Malleable because the lattice can move along and the delocalised
electrons can hold the ions together
Good conductors of heat and electricity because the delocalised electrons have a charge and can move

24
Q

What are Alloys?

A

Metals that are mixed with small amounts of another substance (usually
another metal or carbon)

25
Q

Noble Gasses?

A

Group 18
■ Have full valence shells
■ Are very stable
■ Do not react at all so are referred
to as inert.
■ Glow under particular conditions

26
Q

Halogens?

A

Group 17 non-metals
■ Have all their valence electrons
except one
■ Highly reactive
■ They want to gain that extra
valence electron
■ Fluorine is most reactive

27
Q

Covalent Bonds?

A

The atoms are held together by the
electrostatic attraction between the
positive nucleus and the negative
electrons.
■ This force of attraction is called a
covalent bond.
■ Only valence electrons participate in
covalent bonding. The inner shell
electrons stay around their own atom.
■ Covalent bonds are very strong

28
Q

Forming metal ions?

A

Have 1, 2, or 3 valence electrons
■ So valence shells are at less than
half full
■ “Want” to get rid of their valence
electrons
■ This makes the next inner shell
the valence shell, and it’s already
full
■ Atoms that have lost or gained
electrons are called ions

29
Q

Forming non-metal ions?

A

Non-metals have 4, 5, 6, 7, or 8
valence electrons
■ So valence shells are at least half
full
■ ”Want” to complete their valence
shells

30
Q

Cations?

A

Positive ions are called cations
– Have LOST electrons
– Have more protons than electrons
– Tend to be metals
– Have the same name as the metal

31
Q

Anions?

A

Negative ions are called anions
– Have GAINED electrons
– Have more electrons than protons
– Tend to be non-metals
– Name ends in -ide

32
Q

Where do electrons come from when forming ions?

A

exchanges in chemical reactions

33
Q

Ionic Bonding?

A

Once the ions are formed, the
positive ions are strongly attracted
to the negative ions
■ This attraction is called an ionic
bond
■ Ionic compounds are made of ions
stuck together in massive lattices
■ Ionic bonds are strong but fragile

34
Q

Transition metal ions?

A

Transition metals will often form
more than one ion due to their
complex electron configuration
■ Use roman numerals to show
which ion is used
– Iron (II) oxide = FeO
– Iron (III) oxide = Fe2O3

35
Q

Polyatomic ions?

A

A group of atoms that behaves as a single unit with a specific charge
■ Made up of different atoms in a fixed ratios

36
Q

Writing ionic formula?

A

An ionic formula is the chemical symbol
for the ionic compound
– sodium chloride NaCl
– magnesium fluoride MgF2
■ Some rules:
– The cation is always first, the anion
second
– Total positive charges must equal
total negative charges
– Use subscripts to show the
numbers of each ion
– If you have more than one
polyatomic ion, put it in brackets

37
Q

Monoatomic elements?

A

Metals are usually described as
monoatomic elements, so can be
written as a single chemical
symbol
– silver = Ag
– magnesium = Mg
■ Noble gases are also monoatomic
– neon = Ne
– argon = Ar

38
Q

Diatomic elements?

A

non-metals in groups 14 – 17 do
not exist on their own, described
as diatomic
■ atoms of the element bond with
each other to have full outer shells
and be stable
– oxygen = O2
– nitrogen = N2
– chlorine = Cl2

39
Q

Compounds?

A

When more than one type of atom is
bonded together, these are
represented as a compound
■ Subscripts are used to show more
than one atom of an element
– carbon dioxide = CO2
– sodium chloride = NaCl
– glucose = C6H12O6
■ More than one polyatomic ion is
shown in brackets
– copper nitrate = Cu(NO3)2

40
Q

Conservation of Mass?

A

In a chemical reaction, the mass of the reactants must equal the mass of the products.

41
Q

What is Rate of Reaction?

A

How fast or slow these reactions occur

42
Q

Factors affecting the rate of reactions?

A

The six factors that affect the rate of reactions are:
1. Concentration
2. Pressure
3. Surface area
4. Agitation
5. Temperature
6. Catalysts

43
Q

Concentration?

A

The concentration of a solution is
a measure of the number of
particles per unit volume.
• Concentrated solution = large
number of particles.
• Dilute solution = small number of
particles
Increasing the concentration = increases the rate of reaction.

44
Q

Pressure?

A

Pressure is the number of gaseous
molecules in a given area.
Pressure of gaseous molecules can be
increased by:
• increasing the number of particles
• decreasing the volume of the container
Increasing the pressure = increases the rate of reaction.

45
Q

Surface Area?

A

The surface area of a solid object is the total area
of the outside surfaces of the 3D object.
• Only the particles on the surface of a solid come
into contact with the other reactant when they
react.
• Solid reactants will increase in surface area when
they are cut up into smaller pieces or ground into a
powder. Same volume – increased surface area. Increasing the surface area of a solid = increase in reaction rate.

46
Q

Temperature?

A

When you increase the temperature of a reaction
the rate of reaction also increases.
• An increase in temperature (thermal energy) to
the reaction is converted into kinetic (movement)
energy  particles move at greater speeds.
• Particles are more likely to successfully collide
because they move at faster speed at the
reaction’s activation energy.

47
Q

Catalysts?

A

A catalyst is a substance that can be
added to a chemical reaction to
increase the reaction rate by lowering
its activation energy.
• The catalyst is not a reactant nor a
product of the reaction.
• In the chemical reaction, the catalyst is
written above the reaction arrow
between the reactants and products.

48
Q

Measuring the reaction rate?

A

Rate of reaction can be measured by:
• The speed the reactants are used up.
• The speed the products are formed.

49
Q

Calculating Reaction Rate?

A

= Quantity of reactant used up/time
or
= Quantity of Product formed/time

Physical Science (3 decks)

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