Periodic table

Question 1

Periodic table

Answer 1

Elements in a table with order of increasing atomic number

Question 2

Top of the f block (below transition metals)

Answer 2

Lanthanides

Question 3

Bottom of f block(below transition metals)

Answer 3

Actinides

Question 4

Properties of metals

Answer 4

Shiny solids, good conductors(heat+elec) malleable+ductile, generally high melting and boiling points, react with acid to give off hydrogen gas

Question 5

Metalloids

Answer 5

zigzag down from B including Ge and Sb. Solid at room temp, not malleable or ductile, resist flow of electricity. When in chem reac with metals, they behave like nmetals. When in chem reac with nmetals they behave like metals.

Question 6

Non metals

Answer 6

Dull, brittle, Insulators(Graphite is only exception - it is a conductor). Gaseous nmetals low melting + boiling points. Do not react with acids

Question 7

Metallic nature decreases…

Answer 7

Across the period and increases down a group

Question 8

Metal reactivity increases…

Answer 8

Down a group

Question 9

Non metal reactivity increases…

Answer 9

Up a group

Question 10

Density and melting points increase…

Answer 10

Down a group

Question 11

Non metals become more metallic as…

Answer 11

Down a group

Question 12

Ionization energy

Answer 12

Energy needed per mole to remove e- from an atom in gaseous phase

Question 13

First Ionization energy

Answer 13

energy needed per mole to remove 1st e- from atom in gaseous phase.

Question 14

Successive Ionization energy…

Answer 14

Requires increasing amount of energy to remove successive e- as a result of atom becoming progressively more positively charged from e removed.

Question 15

Noble gases

Answer 15

High ionization energies due to full outer shell which explain why they dont react under normal circumstances

Question 16

Causes of trends in io energy(not first io energy)

Answer 16

Valence electrons get further from nucleus resulting in weaker force of attraction require less energy to remove valence electron from atom and increased shielding effect - core electrons repel valence electrons. More core electrons down a group, shielding effect increases.

Question 17

Electron Affinity

Answer 17

Amount of energy released per mole when an atom or molecule gains an electron to form a negative ion. Halogens most likely to form negative ions. F has highest e affinitiy.

Question 18

Electronegativity

Answer 18

Tendency of atom to attract shared pair of e- to itself. More protons - stronger attraction on a bonding pair of electrons.

Question 19

Ion

Answer 19

Charged particle

Question 20

Cation

Answer 20

Positive ion - lost e-

Question 21

Anion

Answer 21

Negative ion - gained e-

Question 22

Atomic radius

Answer 22

Measure of size of atom

Question 23

Ionic radius

Answer 23

measure of size of cation or anion

Question 24

These increase from left to right across period and decrease as u go down group

Answer 24

Electronegativity, e- affinity and io energy

Question 25

Atomic and ionic radius trends

Answer 25

Bigger as u move down group and smaller across period