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Chemistry > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

1
Q

What is an atom?

A

.Atom is the smallest part of an element that can exist.

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2
Q

What is an element?

A

.An element is a substance of only one type of atom.

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3
Q

How are the elements listed and approximately how many are there?

A

.They are listed in the periodic table, they are approximately 100.

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4
Q

Elements can be classified into two groups based on their properties; what are these groups?

A

.Metals and non-metals.

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5
Q

Elements may combine through chemical reactions to form new products; what are these new substances called?

A

.Compounds.

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6
Q

What is a compound?

A

.Its two or more elements that are chemically combined together in fixed proportions.

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7
Q

Do compounds have the same properties as their constituent elements?

A

.No, they have different properties.

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8
Q

What is a mixture? Does it have the same chemical properties as its constituent materials?

A

. A mixtures has two or more elements that are not chemically combined together.

.A mixture does have the same chemical properties.

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9
Q

What are the methods through which mixtures can be separated (there are five)? Do these involve chemical reactions?

A

.Filtration, crystallization, simple distillation, fractional distillation, and chromatography.

.These methods do not involve chemical reactions.

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10
Q

Describe and explain simple distillation.

A

.Simple distillation is used to separate liquid from a solution.

.The liquid then boils off and condenses in the condenser. So that the thermometer will read the boiling point of the liquid.

.Due to evaporation, we get to keep the liquid.

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11
Q

Describe and explain evaporation

A

.Evaporation is a technique for separating solute from a solvent.

.The solution is heated until the solvent evaporates.

.However, the solute stays in the vessel.

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12
Q

Describe and explain crystallization

A

.Crystallization is a technique for separating some of the solvent by evaporation to form a saturated solution. Then we cool down the solution.

.As we cool down the solution, the solid begins to crystallize, as it becomes less soluble at lower temperatures.

.The crystals can be collected and separated from the solvent via filtration.

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13
Q

Describe and explain fractional distillation.

A

.Fractional distillation is a technique for separating a mixture of liquids. This works when liquids have different boiling points.

.We use a fractionating column that contains glass beads. This helps to separate the compounds.And this allows the mixtures to keep condensing and vaporizing.

.The column is hot at the bottom and cold at the top. The liquid will condense at different heights of the column.

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14
Q

Describe and explain filtration

A

.Filtration is used to separate an insoluble solid from a liquid.

.The insoluble solid ( called a residue) gets caught in the filter paper. This is because the particles are too big to fit through the holes in the paper.

.The filtrate is a substance that comes through the filter paper.

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15
Q

What is the apparatus for filtration?

A

.Filter and funnel.

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16
Q

Describe and explain chromatography

A

.Chromatography is used to separate a mixture of substances dissolved in a solvent.

.In paper chromatography, we place a piece of paper with a spot containing a mixture in a beaker with some solvent .

.The bottom of the paper has to be in contact with the solvent. The solvent level will slowly start to ruse. And separating the spot (mixture) into few spots (components)

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17
Q

What is a separating funnel?

A

. A separatory funnel is an apparatus for separating immiscible liquids.

.Two immiscible liquids of different densities will form two distinct layers in the separatory funnel.

.We can run off the bottom layer ( the liquid with greater density) to a separate vessel.

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18
Q

Describe the plum-pudding model

A

.The atom is a ball of positive charge with negative electron embedded in it.

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19
Q

Describe the Bohr/nuclear model and how it came about

A

.The nuclear model suggests that electrons orbit the nucleus at specific distances (shells)

.It came about from the alpha scattering experiments.

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20
Q

Later experiments led to the discovery of smaller, positive particles in the nucleus; what are these particles called?

A

.Protons

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21
Q

What did the work of James Chadwick provide evidence for?

A

.The existence of neutrons in the nucleus.

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22
Q

Describe the structure of an atom

A

.The all has a small central nucleus that is made up of protons and neutrons around which there are electrons.

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23
Q

State the relative masses and relative charges of the proton, neutron and electron.

A

Masses:
.Protons: 1
.Electrons: Very small
.Neutrons: 1

Charges:
Protons: 1
Electrons: -1
Neutrons: 0

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24
Q

Explain why atoms are electrically neutral.

A

.They have the same number of electrons and protons.

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25
Q

What is the radius of an atom?

A

0.1nm

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26
Q

What is the radius of a nucleus and what is it compared to that of the atom?

A

1 x 10 ^-14

.1/10000

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27
Q

What name is given to the number of protons in the nucleus?

A

.Atomic number.

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28
Q

Atoms of the same element have the same number of which particle in the nucleus?

A

.Protons

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29
Q

Where is the majority of mass of an atom?

A

.The nucleus

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30
Q

What is the mass number?

A

The total number of protons and neutrons.

31
Q

How does one calculate the number of neutrons using mass number and atomic number?

A

.Subtract the atomic number from the mass number.

32
Q

What is an isotope? Do isotopes of a certain element have the same chemical properties?

A

.Atoms of the same element (same proton number) that have a different number of neutrons.

.They have the same chemical properties as they have the same electronic structure.

33
Q

What is the relative atomic mass?

A

.The average mass value which takes the mass and abundance of isotopes of an element into account.

34
Q

Give the electronic configuration of He (2).

A

2

35
Q

Give the electronic configuration of Be (4).

A

2,2

36
Q

Give the electronic configuration of F (9).

A

2,7

37
Q

Give the electronic configuration of Na (11)

A

2,8,1

38
Q

Give the electronic configuration of Ca (20)

A

.2,8,8,2

39
Q

What are ions?

A

Ions are charged particles.

.They are formed when atoms lose electrons (positive ions) or gain electrons (negative ions)

40
Q

Compare the properties of metals and non-metals

A

Metals
.Metals have a high boiling /melting point
.They are good conductors of heat and electricity.
.They are shiny.
.They have great malleability
.They have a high density.
.They form basic oxides.

Non metals
.They have low melting /boiling point
.They are not good conductors of heat and electricity except for graphite
.They are dull.
.They are brittle
.They have a low density
.They form acidic oxides

41
Q

What is formed when a metal reacts with a non-metal?

A

An ionic compound which is made up of positive and negative ions.

42
Q

What is formed when a non-metal reacts with a non-metal?

A

.A molecular compound containing covalently bonded atoms.

43
Q

Explain the following : solute, solvent, solution, miscible, immiscible, soluble, insoluble.

A

.A solute is a substance that can be dissolved in a solvent. Together they form a solution

.Miscible refers to the substance (particularly liquids) that mix together, e.g water and alcohol.

.Water and are immiscible which means they do not mix.

.Soluble refers to the substance that can be dissolved in a solvent e.g. salt in water. Insoluble substance won’t dissolve in a solvent.

44
Q

The columns of the periodic table are called…?

A

Groups

45
Q

The rows of the periodic table are called…?

A

.Periods

46
Q

Are elements in the same group similar or different?

A

.They may have similar chemical properties as they share the same number of outer electrons.

47
Q

In terms of energy levels, what are the differences between elements of the same period?

A

.They have the same number of energy levels.

48
Q

Electrons occupy particular energy levels, with each electrons in an atom at a particular energy level ; which available energy level do electrons occupy?

A

The lowest available energy level.

49
Q

The elements of Group 0 are more commonly known as…?

A

.The noble gases

50
Q

What makes the periodic table periodic?

A

.Similar properties of elements occur at regular intervals

51
Q

Elements in the same group have the same number of electrons in their outer shell ; what does this tell us about their chemical properties?

A

.They have similar chemical properties.

52
Q

In terms of shells, what is the difference between elements in the same period?

A

.They have the same number of shells

53
Q

What change in shell number is seen as one moves down a group?

A

The number of shells increases

54
Q

Early periodic tables were incomplete and elements were placed in inappropriate groups if what was to be followed?

A

.The strict order of atomic weights

55
Q

Knowledge of what made it possible to explain why the order based in atomic weights was not always correct?

A

Isotopes.

56
Q

Mendeleev overcame some problems with the table by doing what? He also changed the order of some elements based on what?

A

.Leaving gaps

.Atomic weights

57
Q

The majority of elements are…?

A

Metals

58
Q

Elements that react to form positive ions are…?

A

.Metals

59
Q

Elements that do not form positive ions are…?

A

Non-metals

60
Q

Elements in Group 1 are known as…?

A

.The alkali metals

61
Q

State three characteristics of the Alkali metals.

A

.They have one electron in their outer shell.
.They have a low density
.They are soft (can be cut with knife).

62
Q

How do Group 1 elements react with non-metals? Why are these reactions similar for the different group 1 elements?

A

.They form ionic compounds which are soluble white solids which form colourless solutions - they all have one electron in their outer shell.

63
Q

How do group 1 elements react with water?

A

.They release hydrogen and form hydroxides which dissolve to form alkaline solutions.

.They also react vigorously with water fizzing and moving around on the surface of the water.

64
Q

How does the reactivity change moving down group 1? Why?

A

.Reactivity increases as the atoms get larger and the distance between the nucleus and the outer electrons increases.

.Thus attraction from the nucleus decreases, allowing them to more easily lose electrons.

65
Q

State five characteristics of Group 7

A

. 7 electrons in the outer shell
.Coloured vapours
.Dioatomic molecules
.Form ionic salts with metals
.Form molecular compounds with non-metals

66
Q

State group 7 elements and the molecules they form.

A

Fluorine, F. F2 is a pale yellow gas
.Chlorine, Cl. Cl2 is a pale green gas
.Bromine, Br. Br2 is dark brown liquid.
Iodine, I. I2 is a grey solid.

67
Q

State three changes that occur in Group 7 as one moves down the group.

A

.Higher relative molecular mass.
.Higher melting and boiling point
.Less reactive - less easily gain electrons.

68
Q

A more reactive halogen displaces a less reactive one from an aqueous solution of its salt; explain the trend in reactivity of halogens in these reactions

A

.Reactivity decreases down the group. As we go down the group, the atoms get larger

.So an incoming electron will be less tightly held by the attractive forces from the nucleus.

69
Q

Compare group 1 metals with transition metals

A

Group 1 metals and transition metals are good conductors of heat and electricity. They are shiny when polished and form ionic compounds with non metals.

.However, transition metals have higher densities and higher melting points than Group 1 elements. They are less reactive and harder than Group 1 metals.

70
Q

State three common characteristics of transition metals

A

.Ions with different charges
.Coloured compounds
.Catalytic properties

71
Q

What is a catalyst?

A

A chemical substance that is used to speed up reactions

72
Q

State the colours of flames observed when lithium, sodium, and potassium burn in oxygen

A

Lithium- Crimson-red
Yellow-orange, Na
Lilac, K

73
Q

Describe the properties of noble gases. Discuss the trends in properties down the group

A

.Non-metals, gases, low boiling points, unreactive

.Have a full outer shell they don’t easily gain or lose electrons

.The boiling point increases down the group, as the atoms get heavier.

Chemistry (1 decks)

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