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Chemistry > Topic 1- Atomic structure and the periodic table > Flashcards

Topic 1- Atomic structure and the periodic table Flashcards

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1
Q

What is an atom?

A

An 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 made from only one type of atom

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3
Q

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

A

They are listed in the periodic table; there are around 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

Two or more elements combined chemically in fixed proportions which can be represented by formulae

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7
Q

Do compounds have the same properties as the 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 mixture consists of two or more elements or compounds not chemically combined together; it does have the same chemical properties

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9
Q

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

A

Filtration, crystallisation, simple distillation, fractional distillation and chromatography; they do not involve chemical reactions

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10
Q

Describe and explain simple distillation

A

Simple distillation is used to seperate liquid from a solution- the liquid boils off and condenses in the condenser. The thermometer will read the boiling point of the pure liquid. Contrary to evaporation, we get to keep the liquid.

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11
Q

Describe and explain crystallisation/evaporation

A

Evaporation is a technique for separation of a solid dissolved in a solvent from a solvent (e.g salt from H20)
The solution is heated until all the solvent evaporates; the solids stay in the vessel
Crystallisation is similar, but we only remove the solvent by evaporation to form a saturated solution (the one where no more solids can be dissolved). Then, we cool down the solution, the soldi starts to crystallise, as it becomes less soluble at lower temperatures. The crystals can be collected and separated from the solvent via filtration.

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12
Q

Describe and explain fractional distillation

A

separation technique that works when liquids have different melting points.
The apparatus is similar to the one of simple distillation apparatus, with the additional fractioning column placed on top of the heated flask
The fractioning column contains glass beads. It helps separate the compounds. In industry, mixtures are repeatedly condensed and vaporised. The column is hot at the bottom and cold at the top. The liquids will condense at different heights of the column.

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13
Q

Describe and explain filtration

A

Filtration is used to separate an insoluble solid is suspended in a liquid.
The insoluble solid (called a residue) gets caught in the filter paper, because the particles are too big to fit through the wholes in the paper.
The filtrate is the substance that comes through the filter paper,
Apparatus; filter paper + funnel

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14
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 rise, thus separating the spot (mixture) into few spots (components)

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15
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.

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16
Q

Describe the plum pudding model

A

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

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17
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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18
Q

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

A

protons

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19
Q

What did the work of James Chadwick provide evidence for?

A

The existence of neutrons in the nucleus

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20
Q

Describe the structure of an atom

A

The atom has a small central nucleus (made up of protons and neutrons) and on the outside shell there are electrons

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21
Q

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

A

Masses: proton = 1 neutron = 1 electron = very small
Charges: proton= 1 neutron = 0 electron = -1

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22
Q

Explain why atoms are electrically neutral

A

They have the same number of electrons and protons

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23
Q

What is the radius of an atom

A

0.1nm

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24
Q

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

A

1x10^-14m and 1/10000

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25
Q

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

A

Atomic number

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26
Q

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

A

protons

27
Q

Where is the majority of mass of an atom?

A

the nucleus

28
Q

What is the mass number

A

The total number of protons and neutrons

29
Q

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

A

Subtract the atomic number from the mass number

30
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

31
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, on a scale where the mass of 12C is 12

32
Q

What are ions?

A

Ions are charged particles. They are formed when atoms lose electrons or gain electrons

33
Q

Compare the properties of metals and non-metals

A

Boiling/melting in metals is high whereas nonmetals have a low melting point
Metals are better conductors of heat and electricity unlike non-metals (with exception of graphite)
metals are shiny, non-metals are dull
non-metals are brittle, metals are stronger
metals have a high density and non-metals have a low density

34
Q

What is formed when a metal and non-metal react?

A

An ionic compund

35
Q

What is formed when a non-metal and a non-metal react?

A

A molecular compound containing covalently bonded atoms

36
Q

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

A

A solute is a substance dissolved in a solvent, together they form a solution
Miscible refers to substances that mix together, immiscible refers to two substances that don’t mix together
Soluble refers to the substance that can’t be dissolved in a solvent. Insoluble substance won’t dissolve in a particular solvent.

37
Q

The columns of the periodic table are called?

A

groups

38
Q

The rows of the periodic table are called?

A

periods

39
Q

Are elements in the same group similar or different?

A

they may have similar chemical properties, as they have the same number pf outer shell electrons

40
Q

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

A

The same number of energy levels

41
Q

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

A

The lowest available energy level

42
Q

The elements of group 0 are more commonly know as?

A

The noble gases

43
Q

What makes the periodic table periodic?

A

Similar properties of elements occur at regular intervals

44
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

45
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

46
Q

The majority of elements are?

A

metals

47
Q

Elements in group 1 are known as?

A

The alkali metals

48
Q

State three characteristics of Alkali Metals

A

One electron in the other shell
Low density
stored under oil
are soft

49
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

50
Q

How do group 1 metals react with water?

A

Release hydrogen and form hydroxides which dissolve to form alkaline solutions; react vigorously with water fizzing and moving around on the surface of the water

51
Q

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

A

Reactivity increases as the the atoms get a larger and the distance between the nucleus and the outer electrons increases and thus attraction from the nucleus decreases, allowing them to more easily loose electrons.

52
Q

State the 5 characteristics of group 7

A

7 electrons in outer shell
coloured vapours
diatomic molecules
form ionic salts with metals
form molecular compounds with non-metals

53
Q

State 5 Group 7 elements and states of matter of molecules they form

A

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

54
Q

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

A

Higher relative molecular mass
higher melting and boiling point
less reactive

55
Q

Compare group 1 metals with transition metals

A

Group 1 metals and transition metals are heat and electricity conductors
Both are shiny when polished
Form ionic compounds with non-metals
Transition metals have higher densities and melting/boiling points than Group 1 metals. They are less reactive and harder than Group 1 metals

56
Q

State three common characteristics of transition metals

A

Ions with different charges
Coloured compounds
Catalytic properties

57
Q

What is a catalyst?

A

A catalyst is a chemical substance that increases the rate of chemical reaction
It is not used up over the course of the reaction

58
Q

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

A

crimson-red, Li
yellow-orange, Na
Lilac, K

59
Q

What did John Dalton describe atoms as?

A

solid spheres, and different spheres made up different elements.

60
Q

In 1879, J J Thompson concluded what from his experiment?

A

Atoms weren’t solid spheres.
His measurements of charge and mass showed that an atom must contain negatively charged particles (electrons)
This new discovery led to the “Plum Pudding Model”

61
Q

What experiment did Ernest Rutherford do in 1909? And what did it conclude?

A

The alpha particle scattering experiment; fired positively charged alpha particles at a thin sheet of gold, expecting the particles to pass straight through the sheet or be slightly deflected at most. Most of the particles did go through, some were deflected more than expected, and a small number were deflected backwards, proving the plum pudding model to be wrong.

62
Q

What did Rutherford come up with to explain the experiment

A

The nuclear model
it stated that there was a positively charged nucleus in the centre of the atom where most of the mass was concentrated, and a cloud of electrons surrounds this nucleus.

63
Q

What did James Chadwick discover?

A

Neutrons

Chemistry (7 decks)

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