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Chemistry > C9 The Periodic Table > Flashcards

C9 The Periodic Table Flashcards

1
Q

How is the periodic table arranged?

A

Elements are arranged on the periodic table in order of increasing atomic number (proton number).

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2
Q

What are periods?

A

Periods are the horizontal rows that show the number of shells of electrons an atom has and are numbered from 1-7.

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3
Q

What are groups?

A

These are the vertical columns that show how many outer electrons (valency electrons) each atom has and are numbered from 1-7 with a final group called Group 0 instead of group 8 -noble gases.

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4
Q

What does valency tell you?

A

Valency tells you how many bonds an atom can make with another atom or how many electrons its atoms lose, gain or share, to form a compound.

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5
Q

How does the group number help determine the charge that metal and non-metal ions form?

A

For metals, the group number corresponds to the number of electrons it will lose to achieve a full outer shell and the charge of the metal ion.
-Metals on left side.
For non-metals, in group 6 and 7, they will gain 1 and 2 electrons respectively to gain a full outer shell.
-Non-metals in group 7 gain 1 electron to form ions with a 1- charge.
-Non-metals in group 6 gain 2 electrons to form ions with a 2- charge.

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6
Q

How does the metallic character of elements change as you move across a period and down a group?

A

The metallic character of elements decreases as you move across a period (left to right) and it increases as you move down a group.

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7
Q

Why does this trend occur? (trend of metallic character)

A

This trend occurs due to atoms more readily accepting electrons to fill their valence shells rather than losing them to have the previous, already full, electron shell as their outer shell.

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8
Q

What lies in between the metals and the non-metals?

A

In between them are elements referred to as metalloids which display some properties of both.

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9
Q

What is the electronic configuration?

A

The electronic configuration is the arrangement of electrons into shells for an atom.

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10
Q

What is the link between the electronic configuration of elements and their position on the periodic table?

A

The number of notations in the electronic configuration will show the number of occupied shells of electrons the atom has, showing the period.
And the last notation shows the number of outer electrons the atom has, showing the group number.

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11
Q

What does the group number show?

A

The group number shows the number of electrons in the outer shell, so all elements in the same group have the same number of outer shells.

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12
Q

How do metals become ions?

A

Metals become positive ions by losing electrons.

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13
Q

How do non-metals become ions?

A

Non-metals become negative ions by gaining electrons.

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14
Q

What are some metallic characters/properties?

A

Metallic properties:
-Malleable
-Conductor of heat and electricity
-Shiny
-High melting and boiling point

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15
Q

What is the group 1?

A

Group 1 are metals that are also called the alkali metals as they form alkaline solutions with high pH values when reacted with water. -first column.

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16
Q

What are the first three members of group 1?

A

-Lithium
-Sodium
-Potassium
These tell us enough about the patterns or trends for us to make predictions of the rest of the group.

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17
Q

Why do group 1 metals react in a similar way?

A

They react in a similar way as they all have one outer electron.

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18
Q

What are the physical properties of the Group 1 metals?

A

The group 1 metals:
-Shiny silvery surfaces when freshly cut.
-Conduct heat and electricity.
-Soft and easy to cut, getting even soften and denser as you move down the Group (sodium and potassium do not follow the trend in density).
-All have low melting points and low densities compared to other metals, and the melting point decreases as you move down the Group.

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19
Q

What happens to the melting point as you go down the group 1?

A

The melting point decreases down group 1.

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20
Q

What happens to the density as you go down the group 1?

A

The density increases going down the group.

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21
Q

How does group 1 react with water?

A

All the metals form a metal hydroxide and hydrogen.
Group 1 metal + water => metal hydroxide + hydrogen

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22
Q

How does lithium react with water?

A

Lithium floats and reacts gently with water.
Bubbles of hydrogen gas.
Lithium + water => lithium hydroxide + hydrogen

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23
Q

How does sodium react with water?

A

Bubbles of hydrogen gas produced. The heat of this causes it to melt into a shiny ball that dashes around surface. Floats on water because it is less dense. White trail of sodium hydroxide produced which dissolves in the water producing a highly alkaline solution.
Sodium + water => sodium hydroxide + hydrogen

24
Q

How does potassium react with water?

A

Reacts very vigorously.
Bubbles of gas, the energy release of this causes it to melt into a shiny ball that dashes around the surface.
Enough heat is produced so it burns with a lilac - coloured flame.
Potassium + water => potassium hydroxide + hydrogen

25
Q

How does reactivity change as you go down group 1?

A

As you go down group 1, the metals get more reactive.
-Rubidium, Caesium and Francium will react more vigorously with air and water.

26
Q

What are the group 7 elements?

A

The group 7 elements are the halogens. They are non-metals that are very poisonous and include iodine, chlorine, bromine…

27
Q

What are halogens? - molecules?

A

Halogens are diatomic meaning they form molecules of two atoms. I2, Cl2, Br2…

28
Q

How many electrons do halogens have in their outer shell?

A

Halogens have 7 electrons in their outer shell. They will need to gain an electron to get a full outer shell.

29
Q

What are the physical properties of the halogens? And how do they change?

A

Physical properties of halogens change down the group (at room temp)
-Darker in colour.
-Melting and boiling points increase.
-Density increases.

30
Q

How does reactivity change down group 7?

A

As you go down group 7, the reactivity decreases.

31
Q

What type of atoms do halogens form?

A

Halogens form halide ions by gaining one more electron to complete their outer shells.

32
Q

What does halide mean?

A

Halide refers to the compounds formed when a halogen combines with another atom, such as a metal.

33
Q

How does the physical state of the halogens change as you go down the group?

A

Chlorine is a pale yellow gas, bromine is a red-brown liquid and iodine is a grey-black solid; This demonstrates that the density of the halogens increase as you go down the group.

34
Q

How does the number of shells of electrons (notations) change as you go down group 7?

A

As you go down group 7, the number of shells of electrons increases. This means that the outer electrons are further away from the nucleus so there are weaker electrostatic forces of attraction which make it harder to attract an incoming electron to complete the full outer shell.

35
Q

How does melting point of halogens change as you go down the group?

A

As you go down group 7, the melting and boiling points increase.
Astatine is at the bottom of group 7 and thus has the highest melting point.

36
Q

How does density of halogens change as you go down the group?

A

As you go down group 7, the density increases.
Fluorine is at top and is a gas.
Astatine is at bottom and is a solid.

37
Q

How does the colour of halogens change as you go down the group?

A

As you go down group 7, the colour of the halogen’s becomes darker.
Fluorine is at top and is very light.
Astatine is at bottom and is black.

38
Q

What is a halogen displacement reaction?

A

A halogen displacement reaction occurs when a more reactive halogen displaces a less reactive halogen form an aqueous solution of its halide.

39
Q

What is group 0?

A

Group 0 are the noble gases. They are non-metals.
They are all monatomic meaning they exist as He, Ne, Ar…
Last column on right hand side of periodic table.

40
Q

What are the melting points like for noble gases?

A

Nobles gases have very low melting and boiling points.

41
Q

What are noble gases in terms of atoms?

A

Noble gases are all monoatomic, colourless gases. - Exist as single atoms such as He, Ne, Ar…

42
Q

Why are noble gases so unreactive and inert?

A

Noble gases are unreactive and inert because they have full outer shells meaning a very stable electronic configuration. They do not easily lose or gain electrons.

43
Q

What does inert mean?

A

Inert is a substance that does not react chemically with any other substance.

44
Q

Why do noble gases have low melting points?

A

They have low melting points because of the weak intermolecular forces of attraction that do not require a lot of energy to break. They are monoatomic and thus have very weak interatomic/intermolecular attractions.

45
Q

How can noble gases be used? Helium for filling balloons.

A

Helium is used in balloons because it is less dense than air so the balloons float and extremely unreactive whereas hydrogen is also light but reactive with air. Helium is also non flammable.

46
Q

How can noble gases be used? Neon in signs.

A

Neon is used in advertising signs because it glows red when a high voltage is passed through.

47
Q

How are noble gases used? Argon in lamps.

A

Argon/krypton/xenon can be used for filament lamps because they stop the oxygen in the light bulbs from corroding the hot tungsten filament.

48
Q

What are the uses of the noble gases? Argon in welding.

A

Argon acts as a shielding gas in welding as it is denser than air so keeps the air off of the metal and inert so metal won”t oxidise.

49
Q

How many electrons do noble gases have in their outer shell?

A

All noble gases except for helium have 8 electrons in their outer shell.
Helium only has 2.

50
Q

Where are the transition elements found?

A

The transition elements are found in the central part of the periodic table and are metals.

51
Q

What are the physical properties of the transition metals?

A

The transition metals are very hard and strong metals.
They conduct heat and electricity.
The transition elements form coloured compounds.

52
Q

What are the melting points of transition elements?

A

Transition elements have high melting points.

53
Q

What is the density of transition elements?

A

The transition elements have high density.

54
Q

What do transition metals often have?

A

Transition metals often have more than one oxidation state, such as iron readily forming compounds of both Fe2+ and Fe3+.

55
Q

What are transition metals used for?

A

Transition metals can be used as catalysts to improve the rest or reaction in industrial processes.

56
Q

What is a catalyst?

A

A catalyst is a substance that increases the rate of reaction without being used up.

Chemistry (9 decks)

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