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Chemistry > Atomic Structure And The Periodic Table > Flashcards

Atomic Structure And The Periodic Table Flashcards

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1
Q

In an atom, what are the particles that are contained?

A

The 3 particles within an atom are protons, neutrons and electrons.

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2
Q

What is the radius of an atom?

A

The radius of an atom is about 0.1 nanometres.

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3
Q

What particles reside in the nucleus of an atom?

A

The neutron and proton can be found in the nucleus of an atom.

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4
Q

What are factors of the nucleus of an atom?

A

The nucleus is in the middle of an atom.
The overall charge of a nucleus is positive.
Almost the entire mass of an atom is concentrated within the nucleus.

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5
Q

State the factors of electrons.

A

Electrons are negatively charged.
Electrons have virtually no mass.
They orbit the nucleus by moving around in their energy levels.

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6
Q

What is similar about protons and electrons?

A

Number of Protons=Number of Electrons

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7
Q

What is the overall charge of an atom?

A

Atoms are neutral.

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8
Q

What is an element?

A

A substance that contains only the same number of protons in its atom.

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9
Q

What are isotopes?

A

Isotopes are different forms of an element, with a varying amount of neutrons.

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10
Q

What is the formula used to identify the relative atomic mass of an element?

A

Relative Atomic Mass=Sum of(isotopes abundance*isotope mass number)/sum of abundace if all the isotopes

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11
Q

What happens when elements react?

A

When elements react, atoms of each element combine with another atom to form a compound.

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12
Q

What is a compound?

A

A substance formed through the reaction of two or more chemically bonded elements.

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13
Q

What is the requirement for forming bonds? (Think about electrons)

A

To form bonds…
Electrons must be given away
Electrons must be shared
Electrons must be taken…by an atom.

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14
Q

What happens when a non-metal and a metal react?

A

The non-metal and metal reacts forming ions. The metal atoms lose electrons to form positive ions whereas the non-metal atoms gain electrons to form negative ions.

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15
Q

What happens when two non-metals react?

A

The two non-metals share bonds between each other (also referred to as covalent bonding).

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16
Q

What is a formula?

A

A formula shows what atoms are in a compound.

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17
Q

What are the molecules on the left side of a reaction called?

A

The reactants are the molecules on the left side of an equation.

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18
Q

What are the molecules on the roght side of an atom called?

A

The products are the molecules on the right side of the equation.

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19
Q

what are mixtures?

A

Mixtures are two or more atoms that are not chemically bonded together.

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20
Q

What methods can be used to separate a mixture?

A

Physical Methods.

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21
Q

Memorise Paper Chromotography.

A

.

22
Q

What does filtration do?

A

It separates insoluble solids from liquids.

23
Q

What are two methods to separate soluble solids from liquids?

A

Crystallisation and Evaporation.

24
Q

How is evaporation carried out?

A

1) Pour the solution into an evaprating dish
2) Slowly heat the solution. The solvent will evaporate as the solution becomes more concentrated
3) Keep heating until dry crystals are left.

25
Q

How do you carry out crystallisation?

A

.

26
Q

What is simple distillation?

A

Simple distillation is a separation technique used to separate out liquids from a solution.

27
Q

What is fractional distillation?

A

Fractional distillation is used to separate a mixture of liquids.

28
Q

What did John Dalton describe the atom to be?

A

A solids sphere that consisted of different spheres each unique to elements.

29
Q

What did J J Thompson conclide from his experiment?

A

J J Thompson invented the plum pudding model. The theory that first introduced electrons.
It presented atoms to be a ball of positive charge with electrons stuck on it.

30
Q

What experiment did Rutherford use to prove the plum pudding model was wrong?

A

Rutherford carried out the gold foil experiment that proved an atom had a positively charged core by shooting alpha particles through it.

31
Q

What conclusion did Rutherford find?

A

Rutherford found out that the alpha particles did go through the gold sheet however he noticed some were deflected away from the sheet.

32
Q

What did Bohr propose?

A

He believed that electrons orbited the nucleus in a fixed shell.

33
Q

In the early 1800s, how were electrons arranged?

A

1) By physical and chemical properties

2) Relative Atomic Mass

34
Q

What did Dmitri Mendeleev do to the periodic table!

A

Dmitri Mendeleev organised elements in order of relative atomic mass. He left gaps in the table of elements that were undiscovered so that in the future they can be replaced.

35
Q

What are metals?

A

Metals are elements that form positive ions when reacting.

36
Q

Which groups are the transition metals found in?

A

The transition metals are found in between group 2 and 3.

37
Q

What are the group 1 elements referred to as?

A

Alkali Metals.

38
Q

What property do all group 1 atoms have in common?

A

They all consist of 1 electron in the atoms outer shell causing them to be extremely reactive.

39
Q

What trends are seen as you go down group 1 atoms?

A

Group 1 atoms:
increase in reactivity
decrease in melting and boiling point
higher relative atomic mass

40
Q

What happens when group 1 element react with water?

A

They react vigorously to produce hydrogen gas and a metal hydroxide.

41
Q

What happens when group 1 elements react with chlorine?

A

They also react vigorously forming a metal chloride salt.

42
Q

What happens to group 1 elemts as they react with oxygen?

A

They form metal oxides.

43
Q

What are the group 7 elements commonly reffered to as?

A

Halogens.

44
Q

What is unique about halogens?

A

They are all non-metals with coloured vapours.

45
Q

What trends occur as you go down group 7?

A

Become less reactive
Higher melting and boiling point
Higher relative atomic mass

46
Q

What type of bonding do halogens undergo?

A

Covalent Bonding

47
Q

What type of ions do halogens form when reacting?

A

Negative charged ions also reffered to as halides.

48
Q

What is uniqie about group 0 elements?

A

They are all inert, colourless gases.

49
Q

What are group 0 elements commonly reffered to as?

A

Noble Gases.

50
Q

What trends are shown as you go down group 0 elements?

A

As you go down group 0 elements
Have increasing boiling points
Increasing relative atomic mass

51
Q

Why do the atoms in noble gases increase in boiling point as you go down on group 0?

A

Due to an increase in electrons leading to a greater intermolecular force between them. to overcome this more energy is needed.

Chemistry (2 decks)

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