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Chemistry - Unit Three > The Periodic Table > Flashcards

The Periodic Table Flashcards

1
Q

What was the first attempt at making a periodic table?

A

Newlands’s Law of Octaves, 1864

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2
Q

How did Newlands present the elements?

A

In order of atomic mass in rows of seven. He said that each eighth element had similar properties so they were put in columns and became known as Octaves.

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3
Q

Why was Newlands’s Law of Octaves criticised?

A
  • Some of his octaves contained elements that didn’t have similar properties
  • He mixed up metals and non-metals
  • He didn’t leave any gaps for undiscovered elements so new elements didn’t fit
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4
Q

How is Mendeleev’s periodic table similar to Newlands’s?

A

They both arrange the elements in order of atomic mass.

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5
Q

How many elements were there in Mendeleev’s original periodic table?

A

60

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6
Q

How was Mendeleev’s periodic table different to Newlands’s?

A

Mendeleev left gaps where the groups didn’t work and predicted the properties of those undiscovered elements.

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7
Q

What was proof that Mendeleev’s periodic table was a success?

A

When new elements were discovered they fitted into the gaps Mendeleev left.

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8
Q

How are elements arranged in the modern periodic table?

A

By atomic number.

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9
Q

What does group number on the periodic table tell us?

A

How many electrons an atom of that elements has on its outermost energy level.

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10
Q

What does period number on the periodic table tell us?

A

The amount of energy levels an atom of that element has.

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11
Q

What is shielding?

A

When lots of inner electrons get in the way of the nuclear charge between the nucleus and electrons.

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12
Q

What effect does shielding have?

A

The more shielding there is (the more full energy shells an atom has), the easier it is for an atom to lose its outermost electrons as it feels a weaker attraction to the nucleus. It also makes it harder for atoms to gain electrons as the attraction of the nucleus is weaker.

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13
Q

What is group one on the periodic table also known as?

A

The alkali metals.

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14
Q

What is the trend with reactivity in the alkali metals?

A

Reactivity goes up the further down the group you go.

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15
Q

What is the trend of melting points and boiling points in the alkali metals?

A

They decrease down the group.

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16
Q

What do the alkali metals react with non-metals to form?

A

Ionic compounds. The alkali metal will become a 1+ ion.

17
Q

What are the products of alkali metals reacting with non-metals usually like?

A

White solids that dissolve in water to form colourless solutions.

18
Q

What is the equation for an alkali metal’s reaction with water?

A

Alkali metal + Water -> Metal Hydroxide + Hydrogen

19
Q

Describe how alkali metals react with water.

A

Vigorously - so much so that the elements below Potassium are explosive.

20
Q

Why are the alkali metals named as such?

A

Because when they react with water the hydroxides made will dissolve in the water to make alkaline solutions.

21
Q

What name is given to the group seven elements?

A

The halogens

22
Q

What is Fluorine like at room temperature?

A

A poisonous yellow gas.

23
Q

What is chlorine like at room temperature?

A

A poisonous dense green gas.

24
Q

What is bromine like at room temperature?

A

A dense, poisonous, red-brown volatile liquid.

25
Q

What is iodine like at room temperature?

A

A dark grey crystalline solid or a purple vapour.

26
Q

True or False: Halogens are diatomic.

A

True

27
Q

What is the trend of reactivity in the halogens?

A

Reactivity decreases down the group.

28
Q

What is the trend of melting and boiling points in the halogens?

A

They increase down the group.

29
Q

What is formed when a halogen reacts with a metal?

A

An ionic compound. A halogen becomes a 1- ion.

30
Q

What is displacement?

A

The ability for a more reactive halogen to remove a less reactive halogen from an aqueous of its salt.

31
Q

Where are the transition metals on the periodic table?

A

The middle.

32
Q

What are two typical properties of transition metals?

A
  • Very conductive

* Dense, strong and shiny

33
Q

What are three differences between the transition metals and the alkali metals?

A
  • Transition metals are a lot less reactive than alkali metals
  • Transition metals are denser, stronger and harder than alkali metals
  • Transition metals have much higher melting and boiling points than alkali metals.
34
Q

What are two facts about ions of transition metals?

A
  • Most can make ions of different charges

* Most form different coloured compounds

35
Q

What is a use of the transition metals in industry?

A

Catalysts

Chemistry - Unit Three (6 decks)

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