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Chemistry Passport > Atomic Structure & Periodic Table > Flashcards

Atomic Structure & Periodic Table Flashcards

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1
Q

Define atom

A

All substances are made from tiny particles called atoms. An atom is the smallest part of an element that can exist.

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2
Q

Define element

A

Contains just one type of atom (e.g oxygen)

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3
Q

Define compound

A

Contains two or more types of atoms joined together (e.g carbon dioxide)

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4
Q

Define mixture

A

Contains two or more different substances not joined together

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5
Q

Combustion (incomplete) equation

A

Fuel + oxygen -> carbon monoxide + water

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6
Q

Combustion (complete) equations

A

Fuel + oxygen -> carbon dioxide + water

Fuel + oxygen -> copper oxide

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7
Q

Balanced equation rules

A

Only change BIG numbers
Can’t change small numbers
Can’t add or take any reactants/products

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8
Q

Balance:

CH4 + 02 -> CO2 + H2O

A

CH4 + 2O2 -> CO2 + 2H2O

C= 1                C= 1 
H= 4               H= 2=4
O= 2=4          O= 3=4
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9
Q

Separating mixtures

What are the methods of this?

A

Filtration is a method for separating an insoluble liquid

Evaporation is a method used to separate a soluble solid from a liquid

Fractional distillation is a method for separating a liquid from a mixture of two or more liquids

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10
Q

Relative mass of proton, neutron and electron

A 
Proton    = 1
Neutron = 1
Electron = almost 0
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11
Q

Relative charge of proton, neutron and electron

A 
Proton   = +1
Neutron=  0
Electron= -1
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12
Q

What is the atomic number and mass number?

A

Atomic number = proton number
Mass number = number of protons + number of neutrons

Tip: neutrons = bigger number - smaller number

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13
Q

What is the radius of an atom?

A

About 0.1nm (1x10^-10m)

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14
Q

What are subatomic particles?

A

Protons, neutrons and electrons

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15
Q

Size and scale equation

A

Larger value/smaller value

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16
Q

What is electronic configuration?

A

The arrangement of electrons in these shells is often called the electronic configuration

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17
Q

Explain how group and period number are related to electron structure

A

In the modern periodic table, elements are in order of atomic number in periods and groups. Electronic configurations/structure are arranged in atoms

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18
Q

Does the atomic number increase as you move down a group or across a period?

A

Yes

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19
Q

Explain how the position of elements in the periodic table is related to the arrangement of electrons

A

The number of electrons in the outer shell of an element is represented in the periodic table as the group number that element is situated in

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20
Q

Explain the differences between metals and non metals

A

Metal properties: malleable, shiny, good conductors of heat/electricity, high melting/boiling point.

Non metal properties: brittle, dull/matte, good insulators (poor conductors), tends to be liquids/gases.

Metals are located on the left of the periodic table, and non metals are located on the upper right.

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21
Q

Compare the position of subatomic particles in the plum pudding model with the nuclear model (4 marks)

A
  • the nuclear model has electrons in shells, the plum pudding doesn’t
  • the plum pudding doesn’t have a nucleus, but the nuclear model does
  • the plum pudding model has a ball of positive charge, but the nuclear model has a positive nucleus only
  • they both have electrons
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22
Q

Explain how the plum pudding, nuclear and Bohrs models were developed

A

^ Nuclear -> discovered nucleus
| Bohr’s -> he showed that electrons occupy shells or energy levels around the nucleus
| Plum P -> tiny spheres that can’t be divided

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23
Q

Describe why the new scattering experiment led 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

This led to the plum pudding model being replaced by the nuclear model

24
Q

Describe the development of the periodic table

A

In 1868, Russian chemist, Dimitri Mendeleev, started the development of the periodic table,
arranging chemical elements by atomic mass

He predicted the discovery of other elements, and left spaces open for them

25
Q

Explain how scientists knew certain elements were in incorrect groups

A

Scientists thought Mendeleev’s table was incorrect, because group 4 contained metals to place elements and non metals not known at the time

26
Q

What are the physical differences between metals and non metals (name 3 each)

A 
Metals: 
Shiny
High melting points 
Good conductors of heat/electricity 
High density 
Malleable & ductile 
Non metals:
Dull
Low melting points/usually liquids or gases
Good insulators 
Low density 
Brittle
27
Q

What are the chemical differences between metals and non metals

A

Metals form oxides that are basic, but non metals form oxides that are acidic

Metals react with water and oxygen, to create oxides, non metals don’t react with water

28
Q

Explain how the reactions of elements are related to the arrangement of electrons in their atoms

(and hence their atomic)

A

The elements in the periodic table are arranged in order of atomic number
so that elements with similar properties are in columns, known as groups.
The table is called a periodic table because similar properties occur at regular intervals

Elements in the same group in the periodic table have the same outer shell, and this gives them similar chemical properties

29
Q

Describe the reactions of the first 3 alkali metals with oxygen, water & chlorine

Group 1 - the alkali metals

A

The group 1 elements are all soft, reactive metals with low melting points.
They react with water to produce an alkaline metal hydroxide solution and hydrogen

The alkali metals react with group 7 metals, like chloride (as they can lose electron to make a full shell, and group 7 need to gain one to make a full shell)

30
Q

Oxygen: reacts to ______ in the air. E.g Sodium burn in the air with _________ flame, forming Sodium oxide.

A

Oxygen

Yellow

31
Q

Water: react with ______ to produce a metal hydroxide and __________.

E.g sodium reacts with water to make sodium hydroxide and _________.

Sodium hydroxide is an ________. It’s a base that _________ in water to form an alkaline solution.

A

Water
Hydrogen

Hydrogen

Alkali
Dissolves

32
Q

Describe the nature of the compounds formed when chlorine, bromine and iodine react with metals and non metals

A

The group 7 elements are known as halogens.

They are reactive non metals and are always found in compounds with other elements.

Chlorine, bromine and iodine are all halogens.

33
Q

The non metal elements in group 7 get ______ reactive as you go down the group, this is an _______ trend to group 1.

A

Less

Opposite

34
Q

Fluorine is the ______ reactive element of all in Group _.

A

Most

7

35
Q

The _____ reactive halogen displaces all of the other halogens from solutions of their salts, and itself displaced by non of the others.

A

Most

36
Q

Chlorine water

Is added to three solutions: potassium chloride, potassium bromide, potassium iodine.

The chloride has __ reaction, the bromine has d________ and the iodine has d________.

A

No
Displacement
Displacement

37
Q

Bromine water

Is added to the three solutions (p chloride , p bromine, p iodine).

The bromine has ____ reaction, the chloride has ____ reaction and the iodine has _________.

A

No
No
Displacement

38
Q

Iodine water

Is added to the three solutions (chloride, bromine and iodine).

They all have _______ reaction.

A

No

39
Q

Explain how properties of the elements in group 0 depend on their outer shell of electrons if the atoms

A 
Group 0 (noble gases)
The atoms of noble gases already have complete outer shells, so they have no tendency to lose, gain or share electrons
40
Q

Explain how properties of the elements in group 1 depend on their outer shell of electrons if the atoms

A

Alkali metals react vigorously with water to produce an alkaline solution.

In a reaction, an atom of a group 1 element will form an ion with a single positive charge.

E.g sodium forming sodium ion. A change like this, where an electron is lost is an example of oxidisation. The ions formed have a stable electronic structure, like a noble gas.

41
Q

Explain how properties of the elements in group 7 depend on their outer shell of electrons if the atoms

A

Further down the group, the atoms have more shells of electrons, so the outer shell containing electrons is further from positive attraction of the nucleus.

This means the force of attraction between the positive nucleus and an incoming electron decreases as they’re less reactive.

42
Q

Predict properties from given trends down the group 0

A

As you go down group 0, the noble gases

boiling point increases,

the density increases,

the atomic radio increases

and the atomic number increases

because extra electron shells are successfully added.

43
Q

Predict properties from given trends down the group 1

A

As you go down group 1, the atom gets bigger.

The bigger the atom, the further away the last electron.

Therefore, the attraction between the nucleus and the last electron gets weaker.

This makes it easier for the atom to give up the electron which increases its reactivity.

44
Q

Predict properties from given trends down the group 7

A

As you go down group 7, volatility decreases as the boiling points increase.

The halogens get less reactive.

Nuclear charge increases, so the nuclear attraction on the outer electrons are stronger.

Electron shielding increases and outweighs the nuclear attraction.

45
Q

Halogens

As you increase the atomic number, the melting and boiling point __________. As you go down the group, ________ decreases.

A

Increases

Reactivity

46
Q

Noble gases

Full ___ shell - don’t _____ with others.

They’re all very ________.

A

Outer
React

Unreactive

47
Q

Noble gases

As you increase the atomic number the boiling point _______.

A

Increases

48
Q

Particle diagrams

Give the ideas about how _____ particles are to each other.

Clear which states have most and least _______.

Doesn’t show the _______ between the particles.

Looks like each particle is a “_____”.

A

Close

Energy

Forces

Solid

49
Q

Forces hold _____ (atoms/ions/molecules) together.

Strong forces need lots of _____ for them to ________.

Weak forces need little _______ for them to be _______.

A

Particles

Energy
Overcome

Energy
Overcome

50
Q

Bigger particles = _______ forces

Smaller particles = _______ forces

A

Stronger

Weaker

51
Q

High boiling point (_____ at room temp)

_______ structures
________ forces holding the particles together
Takes lots of ______ to overcome (break these)

A

Solid

Giant
Strong
Energy

52
Q

Low boiling point (_______ at room temp)

______ forces holding the particles together
_______ structures
Takes not much ______ to overcome (break) these

A

Gas

Weak
Small
Energy

53
Q

Explain why fluorine is a gas at room temperature

A

The forces between molecules are weak, so they require little energy to break them.

Molecules are small.

54
Q

Potassium fluoride is an ionic compound

Explain why ionic compounds have high melting points

A

Because there’s a strong force of attraction.

Meaning a large amount of energy is needed to break these.

Giant structures.

55
Q

Explain why calcium fluoride has a high melting point

A

Giant structure.

Strong forces of attraction/ionic bonds.

Need lots of energy needed to overcome it.

Chemistry Passport (4 decks)

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