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Chemistry > the periodic table > Flashcards

the periodic table Flashcards

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1
Q

How are elements ordered in the modern periodic table? ★

A

By their atomic/proton number.

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2
Q

What are periods? What do elements in each period have in common? ★

A

Horizontal rows in the periodic table; elements in each row have the same number of shells.

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3
Q

What are groups? What do elements in each group have in common? ★

A

Vertical columns in the periodic table; elements are grouped by the same number of electrons in their outermost shell.

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4
Q

What are the majority of elements? ★

A

Metals.

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5
Q

Where are metals and non-metals found on the periodic table? ★

A

● Metals: to the left side and towards the bottom of the Periodic Table.
● Non-metals: to the right side and towards the top of the Periodic Table.

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6
Q

How were elements ordered in the old periodic table? Why was this a problem?

A

By their relative atomic masses; isotopes were a problem because of this.

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7
Q

How did Newland order elements? ★

A

He ordered them in increasing atomic weight, where every 8th element had similar properties and reacted similarly.

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8
Q

How did Mendeleev order elements? What else did he do? ★

A
  1. He ordered them in increasing relative atomic mass as protons not been discovered yet.
  2. He switched the order of certain elements so they fitted patterns of properties of other elements in same group.
  3. He left gaps for undiscovered elements (group 0 not been discovered) and predicted their properties using other elements - was correct.
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9
Q

What enabled the order of the periodic table to be changed?

A

Knowledge of isotopes explained why the order based on atomic weight wasn’t always correct.

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10
Q

What are the properties of metals? (6)

A

● Boiling/melting points: mostly high
● Conductivity: good, heat/electricity
● Appearance: lustrous
● Ductility: yes
● Malleability: yes
● Oxides: basic

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11
Q

What do positive ions do?

A

They lose electrons.

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12
Q

What do negative ions do?

A

They gain electrons.

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13
Q

What is group 1 called? ★

A

Alkali metals.

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14
Q

What is the chemical equation of alkali metals and water? What may you observe? ★

A

A. metal + Water —> Metal hydroxide + Hydrogen gas.
● They react vigorously with water fizzing and moving around on the surface of the water..

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15
Q

What is the chemical equation of alkali metals and oxygen? What may you observe? ★

A

A. metals + Oxygen = White metal oxides.
● Colour of flames: Li = crimson-red, Na = yellow-orange, K = lilac.

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16
Q

What is the chemical equation of alkali metals and green chlorine gas? What may you observe? ★

A

A. metal + Green chlorine gas = White metal chloride salts.

17
Q

Which elements in group 1 have a low density + float in water?

A

● Lithium (Li).
● Sodium (Na).
● Potassium (K).

18
Q

What are the trends reactivity in group 1? Why is this a trend? ★

A

Reactivity increases going down the group.
● This is due to the outer-shell electrons becoming further away from the nucleus as you go down the group.
● So the nuclear attraction weakens.
● There’s more shielding.
● The electron is easier to lose.

19
Q

What is group 0 called? ★

A

Noble gases.

20
Q

What is the reactivity of noble gases? Why? ★

A

They are unreactive and don’t easily form molecules; due to their atoms having a full outer shell of electrons, making them stable them stable.

21
Q

What are the properties in group 0? Why? ★

A

● Boiling point increases going down the group; There are stronger intermolecular attractions between electrons that need to be overcome.

22
Q

What is group 7 called?

A

Halogens.

23
Q

Are halogens metals or non-metals?

A

Non-metals.

24
Q

What do halogens form when reacting together?

A

Diatomic molecules (molecules with two atoms) joined together with a covalent bond.

Diatomic: consists of molecules made of pairs of atoms.

25
Q

What are the properties of halogens going down the periodic table?

A

● Relative molecule mass increases.
● Melting point increases.
● Boiling point increases.

26
Q

What are the trends in group 7?

A

● Reactivity decreases going down.
● This is due to the outer shell electrons becoming further away from the nucleus.
● So the nuclear attraction weakens.
● Electron is harder to gain.

27
Q

What are the appearances of Fluorine, Chlorine, Bromine and Iodine?

A

● Fluorine (F) = yellow gas.
● Chlorine (Cl) = green gas.
● Bromine (Br) = red-brown volatile liquid.
● Iodine (I) = dark grey solid/purple vapour.

28
Q

What is displacement?

A
  1. When a more reactive element/metal displaces a less reactive element/metal in a reaction.
  2. When a more reactive halogen displaces a less reactive halogen from an aqueous solution of its salt.
29
Q

What are the properties of transition metals?

A

● Hard and strong.
● High density.
● High melting points (except mercury).
● Less reactive than group 1 metals (e.g. with oxygen, chlorine, water).
● Good conductors.

30
Q

What ions do transition metals have?

[example included]

A

Ions with different charges noted by the roman numerals.

e.g. Fe (III) = Fe3+

31
Q

What compounds do transitions metals form? What can they be used as?

A

● Coloured compounds.
● Can be used as catalysts to speed up chemical reactions.

32
Q

What did Doberoëiner notice about the periodic table? ★

[include example]

A

Elements with similar chemical properties often occurred in three’s (triads).

e.g, lithium, sodium, potassium all are heavily reactive in water.

33
Q

What are the properties of group 1?

state 5 facts.

A

● Soft metals (can be cut with a knife)
● Relatively low melting points
● Low density (Li, Na, K = less dense than water)
● React rapidly with oxygen, chlorine, water
● Form +1 ions e.g., Na+

34
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.

35
Q

What are the properties of non-metals? (6)

A

● Boiling/melting points: low
● Conductivity: don’t (except graphite)
● Appearance: dull
● Ductility: no
● Malleability: brittle
● Oxides: acidic

Chemistry (16 decks)

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