C2+ Periodic Table

Question 1

What does periodic mean?

Answer 1

Appearing or occurring at intervals.

Question 2

How were elements originally classified before discovery of protons, neutrons, and electrons?

Answer 2

By arranging them in order of their atomic weights.

Question 3

What was the problem with early periodic tables based strictly on atomic weights?

Answer 3

They were incomplete and some elements were placed in inappropriate groups.

Question 4

What did Dobereiner suggest for classifying elements?

Answer 4

Triads (groups of 3).

Question 5

What is Newlands’ law of octaves?

Answer 5

A classification where elements repeated properties every eighth element; it worked only for the first 20 elements.

Question 6

How did Mendeleev improve the periodic table?

Answer 6

By leaving gaps for undiscovered elements and sometimes changing the order based on atomic weights.

Question 7

What did Mendeleev’s predictions about undiscovered elements lead to?

Answer 7

Elements with predicted properties were discovered and filled the gaps.

Question 8

How did knowledge of isotopes explain problems with ordering elements by atomic weight?

Answer 8

It showed why the strict atomic weight order was not always correct.

Question 9

What is Group 1 in the periodic table called?

Answer 9

Alkali metals.

Question 10

Why do Group 1 metals have characteristic properties?

Answer 10

Because they have one electron in their outer shell.

Question 11

What happens when Group 1 metals react with chlorine?

Answer 11

They burn with a bright flame to make a white solid.

Question 12

How does reactivity change down Group 1?

Answer 12

Reactivity increases going down the group.

Question 13

Why does reactivity increase down Group 1?

Answer 13

Outer electron is further from nucleus, more shielding, so electron is more easily lost.

Question 14

What happens when lithium reacts with water?

Answer 14

It fizzes, floats, and releases hydrogen gas.

Question 15

What happens when sodium reacts with water?

Answer 15

It fizzes faster, floats, melts into a ball, and releases hydrogen gas.

Question 16

What happens when potassium reacts with water?

Answer 16

It bursts into a purple flame and releases hydrogen gas.

Question 17

What is Group 7 called?

Answer 17

The halogens.

Question 18

Why do halogens have similar reactions?

Answer 18

Because they all have seven electrons in their outer shell.

Question 19

Are halogens metals or non-metals?

Answer 19

Non-metals.

Question 20

What form do halogen molecules take?

Answer 20

Molecules made of pairs of atoms.

Question 21

How do relative molecular mass, melting point, and boiling point change down Group 7?

Answer 21

They increase going down the group.

Question 22

How does reactivity change down Group 7?

Answer 22

Reactivity decreases going down the group.

Question 23

Why does reactivity decrease down Group 7?

Answer 23

More shielding and outer electron is further from the nucleus, so it is harder to gain.

Question 24

What can a more reactive halogen do in aqueous solution?

Answer 24

Displace a less reactive halogen from its salt solution.

Question 25

What is fluorine’s state and color?

Answer 25

Pale green gas.

Question 26

What is chlorine’s state and color?

Answer 26

Pale yellow-green gas.

Question 27

What is bromine’s state and color?

Answer 27

Red brown liquid.

Question 28

What is iodine’s state and color?

Answer 28

Grey solid that sublimes into a purple vapour.

Question 29

What is astatine’s state and color?

Answer 29

Black radioactive solid.

Question 30

What are Group 0 elements called?

Answer 30

Noble gases.

Question 31

Are noble gases reactive or inert?

Answer 31

Inert (unreactive).

Question 32

Why are noble gases unreactive?

Answer 32

Because their atoms have stable arrangements of electrons.

Question 33

How many electrons are in the outer shell of noble gases?

Answer 33

Eight electrons, except helium which has two.

Question 34

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

Answer 34

Boiling points increase with increasing relative atomic mass.

Question 35

What does compare mean?

Answer 35

Describe similarities and/or differences between things, not just write about one.

Question 36

What are transition elements?

Answer 36

Metals with similar properties that differ from Group 1 elements.

Question 37

How do Group 1 metals differ from transition metals?

Answer 37

Group 1 metals have lower melting points, are softer, and more reactive.

Question 38

What properties do both Group 1 and transition metals share?

Answer 38

Both conduct heat and electricity.

Question 39

What kind of compounds do Group 1 metals make?

Answer 39

Only white compounds.

Question 40

What kind of compounds do transition metals make?

Answer 40

White and coloured compounds.

Question 41

What special properties do many transition elements have?

Answer 41

Ions with different charges, form coloured compounds, and are useful as catalysts.

Question 42

Compare the reactions of lithium, sodium, and potassium with water.

Answer 42

Lithium fizzes and floats. Sodium fizzes faster, floats faster, and melts into a ball. Potassium reacts even faster, floats, and bursts into a purple flame.

Question 43

Why does reactivity increase from lithium to potassium?

Answer 43

Outer electron is further from the nucleus and more shielded, so it's lost more easily.