Periodic Table retrieval questions Flashcards

1
Q

How is the modern Periodic Table ordered?

A

by atomic number

The modern Periodic Table is arranged in order of increasing atomic number.

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2
Q

How were the early lists of elements ordered?

A

by atomic mass

Early versions of the Periodic Table were organized based on atomic mass.

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3
Q

Why did Mendeleev swap the order of some elements?

A

to group them by their chemical properties

Mendeleev rearranged elements to better reflect their chemical behavior.

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4
Q

Why did Mendeleev leave gaps in his Periodic Table?

A

leave room for elements that had not yet been discovered

Mendeleev predicted the existence of undiscovered elements.

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5
Q

Why do elements in a group have similar chemical properties?

A

have the same number of electrons in their outer shell

The outer shell electron configuration determines chemical properties.

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6
Q

Where are metals and non-metals located on the Periodic Table?

A

metals to the left, non-metals to the right

This arrangement highlights the distinction between metals and non-metals.

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7
Q

What name is given to the Group 1 elements?

A

alkali metals

Group 1 elements are known for their reactivity, particularly with water.

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8
Q

Why are the alkali metals named this?

A

they are metals that react with water to form an alkali

Alkali metals produce hydroxides when they react with water.

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9
Q

Give the general equations for the reactions of alkali metals with oxygen, chlorine, and water.

A
  • metal + oxygen → metal oxide
  • metal + chlorine → metal chloride
  • metal + water → metal hydroxide + hydrogen

These reactions demonstrate the typical behavior of alkali metals.

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10
Q

How does the reactivity of the alkali metals change down the group?

A

increases (more reactive)

Reactivity increases due to the increasing atomic size down the group.

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11
Q

Why does the reactivity of the alkali metals increase down the group?

A

they are larger atoms, so the outermost electron is further from the nucleus

Increased distance from the nucleus results in weaker attraction for the outermost electron.

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12
Q

What name is given to the Group 7 elements?

A

halogens

Halogens are known for their reactivity and tendency to form salts.

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13
Q

Give the formulae of the first four halogens.

A

F₂, Cl₂, Br₂, I₂

These are the diatomic molecular forms of the first four halogens.

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14
Q

How do the melting points of the halogens change down the group?

A

increase (higher melting point)

Halogens exhibit an increase in melting points as you move down the group.

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15
Q

How does the reactivity of the halogens change down the group?

A

decrease (less reactive)

Reactivity decreases due to the increasing atomic size and shielding effect.

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16
Q

Why does the reactivity of the halogens decrease down the group?

A

they are larger atoms, so the outermost shell is further from the nucleus

The increased distance makes it harder for halogens to gain an electron.

17
Q

What is a displacement reaction?

A

when a more reactive element takes the place of a less reactive one in a compound

This type of reaction is common in halogen chemistry.

18
Q

What name is given to the Group 0 elements?

A

noble gases

Noble gases are characterized by their lack of reactivity due to full outer electron shells.

19
Q

Why are the noble gases inert?

A

they have full outer shells so do not need to lose or gain electrons

This electron configuration leads to their chemical stability.

20
Q

How do the melting points of the noble gases change down the group?

A

increase (higher melting point)

The trend in melting points reflects the increase in atomic size and mass.