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chemistry 1 > ATOMIC STRUCTURE AND PERIODIC TABLE > Flashcards

ATOMIC STRUCTURE AND PERIODIC TABLE Flashcards

1
Q

Describe simple distillation

A

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

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2
Q

Explain distillation

A

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

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3
Q

Describe and explain evaporation

A

Evaporation is a technique for separation of a solid solute in a solution.
The solution is heated until all the solvent evaporates;the solid stays in the vessel

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4
Q

Describe and explain crystallisation

A

Crystallisation is a separation technique that is used to separate a solid that has dissolved in a liquid and made a solution.

The solution is warmed in an open container,
allowing the solvent to evaporate, leaving a saturated solution.
A solution that has as much solid dissolved in it
as it can possibly contain is called a saturated solution.

As the saturated solution is allowed to cool,
the solid will come out of the solution and crystals will start to grow.
The crystals can then be collected and allowed to dry.

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5
Q

Describe fractional distillation

A

Fractional distillation is used to separate a mixture of liquids.it works when they have different boiling points

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6
Q

Describe filtration

A

It is used to separate an insoluble solid that is in a liquid. filter paper is placed in a glass funnel and a container beneath
The mixture of the solid and liquid is placed into the filter paper.
The liquid flows through the filter paper and in to the container.
The liquid in the container is called the filtrate.

The solid that remains in the filter paper is called the residue.

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7
Q

Describe chromatography

A

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

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8
Q

Explain what happens during chromatography

A

In paper chromatography, we use a paper with a spot containing a mixture in a beaker with some solvent.The bottom of the paper has to be in contact with solvent.The solvent level will slowly rise,thus separating the spot(mixture)into few spots(components)

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9
Q

What is a separating funnel

A

An apparatus for separating unmixable liquids

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10
Q

What positive particle in nucleus was discovered later on

A

protons

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11
Q

What did the work of james chadwick provide evidence for

A

Neutrons in the nucleus

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12
Q

Describe the structure of an atom

A

The atom has a small central nucleus (made up of protons and neutrons)around which are electrons

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13
Q

State relative masses and charges of proton,neutron and electron

A

proton:1,+1
neutron:1,0
electron:very small,-1

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14
Q

Explain why atoms are electrically neutral

A

They have the same number of electrons and protons

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15
Q

What is radius of an atom

A

0.1 nm

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16
Q

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

A

Atomic number

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17
Q

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

A

PROTONS

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17
Q

What is the mass number

A

The total number of protons and neutrons

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18
Q

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

A

Subtract the atomic number from the mass number

19
Q

What is an isotope

A

Atoms of the same element (same proton number) but different number of neutrons

20
Q

Do isotopes have same chemical properties

A

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

21
Q

Give electronic configurations of F(9) AND Na(11)

A

F=2,7 Na=2,8,1

22
Q

What are ions

A

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

23
Q

What is a solvent
What is miscible

A

A solute is a substance that is dissolved in a solvent.Together, forming a solution.
Miscible refers to substances that mix together e.g. water and alcohol

24
Q

what does soluble mean

A

soluble refers to the substance that can be dissolved in a solvent e.g. salt in water.

25
Q

Why are elements in the same group similar

A

They have similar chemical properties ,as they have same number of electrons on outer shell

26
Q

State 3 characteristics of alkali metals

A

All have one electron in the outer shell ;have low density;are soft can be cut with knife

27
Q

How do group 1 elements react with non-metals?

A

They form ionic compounds which are soluble white solids which form colourless solutions.
Reactions are similar for all group 1 metals as they have 1 electron in outer shell

28
Q

How do group 1 elements react with water

A

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

29
Q

How does reactivity change moving down group 1?

A

Reactivity increase as atoms get larger and distance between nucleus and outer electrons increase and thus attraction from nucleus decreases allowing them to easily lose more electrons

30
Q

State 3 group 7 metals and the states of matter of molecules they form

A

Flourine,F. F2 is a pale yellow gas
Chlorine,Cl. Cl2 is a pale green gas
Bromine,Br.Br2 is a dark brown liquid

31
Q

State 3 changes that occur as you go down group 7

A

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

32
Q

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

A

Reactivity decreases down the group.As we go down the group, atoms get larger,so an incoming electron will be less tightly held by the attractive forces from nucleus.This is why Cl2 displaces Br- and I-

33
Q

State 3 common characteristics of transition metals

A

Ions with different charges
coloured compounds
catalytic properties

34
Q

Describe the properties of noble gases

A

Non-metals,gases,low melting points,unreactive,full outer shell
Boiling point increases as you go down as atoms get heavier

35
Q

why did new evidence from the scattering experiment lead to a change in the atomic model

A

The results from the alpha scattering experiment led to the conclusion that the mass of an atom was concentrated at the centre (nucleus) and that the nucleus was charged

36
Q

explain how the position of an element in the periodic table is related to the arrangement of electrons in its atoms and hence to its atomic number

A

Moving through the elements in the periodic table, each atom has one more electron than the last because the number of electrons is the same as the atomic number . Electrons occupy the shells in order, starting with the shell that is nearest the nucleus

37
Q

how to predict possible reactions and probable reactivity of elements from their positions in the periodic table.

A

The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity. Period - reactivity increases as you go from the left to the right across a period. Group
reactivity decreases as you go down the group.

38
Q

explain the differences between metals and non-metals on the basis of their characteristic physical and chemical properties.

A

metals:shiny,high melting points, good conductors of electricity,good conductors of heat
non-metals:dull,low melting point, poor conductors of electricity, poor conductors of heat

39
Q

explain how the reactions of elements are related to the
arrangement of electrons in their atoms and hence to their
atomic number

A

the nature of the reactions which occur depend upon the number of outer shell electrons in the reacting atoms

40
Q

explain how properties of the elements in Group 0 depend on the outer shell of electrons of the atoms

A

This means that they have no tendency to lose, gain, or share electrons

41
Q

explain how properties of the elements in Group 1 depend on the outer shell of electrons of the atoms

A

The atoms of all group 1 elements have similar chemical properties and reactions because they all have one electron in their outer shell

42
Q

explain how properties of the elements in Group 7 depend on the outer shell of electrons of the atoms

A

They need to gain one electron to make a full outermost shell.

43
Q

predict properties from given trends down the group7

A

As you go down group 7, the relative atomic mass increases and the boiling point of halogens also increases.

44
Q

describe the difference in transition metals compared with Group 1 in melting points, densities, strength, hardness

A

Transition metals are much stronger, denser and harder than the group 1 elements. Their melting points are also much higher

45
Q
A

chemistry 1 (2 decks)

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