The Periodic Table

Question 1

Triad

Answer 1

Group of 3 elements with similar properties

Question 2

Mendeleev’s Periodic Table

Answer 2

Created in 1869, he organized the elements in increasing atomic mass

Question 3

Henry Moseley’s Periodic Table

Answer 3

Created in 1913, he organized the elements in increasing atomic number

Question 4

Periodic Law

Answer 4

When elements are arranged in order of
increasing atomic number, there is a periodic repetition of their physical and chemical properties

Question 5

Groups

Answer 5

Columns of elements that share similar properties and have the same number of valence electrons

Question 6

Periods

Answer 6

Horizontal rows of elements that don’t have similar properties. The first element in a period will be a reactive metal, and the last a stable gas

Question 7

Hydrogen

Answer 7

A group of it’s own. A gas at room temperature, 1 energy level, 1 valence electron, and an electron configuration ending in 1s1

Question 8

Representative Elements

Answer 8

Groups 1A-7A. Have a wide range of chemical and physical properties

Question 9

Alkali Metals

Answer 9

Group 1, 1 valence electron, configuration ends in s1. Shiny, clay consistency, cut easily, most reactive metals

Question 10

Alkaline Earth Metals

Answer 10

Group 2, 2 valence electrons, configuration ends in s2. Never found free in nature

Question 11

Transition Metals

Answer 11

Elements in the B groups, configurations end in d1-d10, have 1 or 2 valence electrons. Goods conductors

Question 12

Transition Elements

Answer 12

Have properties similar to each other and other metals, but their properties don’t fit with any other group

Question 13

Lanthanides and Actinides

Answer 13

Configurations end in f1-f14. Known as the inner transition series because of the position in the middle of the transition metals

Question 14

Boron Family

Answer 14

Found in the 13th column or 3A, 3 valence electrons, configurations end in p1

Question 15

Carbon Family

Answer 15

Found in the 14th column or 4A, 4 valence electrons, configurations end in p2

Question 16

Nitrogen Family

Answer 16

Found in the 15th column or 5A, 5 valence electrons, configurations end in p3

Question 17

Chalcogen Family

Answer 17

Found of 16th column or 6A, 6 valence electrons, configurations end in p4

Question 18

Halogen Family

Answer 18

Found in the 17th column or 7A, 7 valence electrons, configurations end in p5. Most reactive non-metals

Question 19

Noble Gas family

Answer 19

Found in the 18th column or 8A, 8 valence electrons- a full octet, most stable elements, rarely bond to others, configuration ends in p6

Question 20

Properties of metals

Answer 20

Conductors, shiny, ductile, rusts, most are solids, and malleable

Question 21

Properties of non-metals

Answer 21

Not good conductors, dull, most are gases, and not ductile or malleable

Question 22

Properties of metalloids

Answer 22

Have the properties of metals and non-metals

Question 23

Melting point

Answer 23

Temperature at which an element melts

Question 24

What happens to melting point as you go down a column?

Answer 24

It increases

Question 25

What happens to melting point as you move to the center of the table

Answer 25

It increases

Question 26

How does force of attraction increase?

Answer 26

It increases with ionization energy and electron affinity due to shielding

Question 27

Shielding

Answer 27

When more inner electrons are close to the nucleus and are attracted to it, this makes the valence electrons easier to remove

Question 28

Ionization energy

Answer 28

Energy needed to remove an electron from the ground state of an atom or ion

Question 29

What happens to ionization energy moving down a column?

Answer 29

It decreases because atomic size increases, making electrons easier to remove

Question 30

What happens to ionization energy moving across a period?

Answer 30

It increases because atomic size increases, making there more attraction, and making it harder to remove electrons

Question 31

First ionization energy, second ionization energy, etc.

Answer 31

The amount of energy it takes to remove the first valence electron, then the second, and so on. Each successive electron takes more energy to remove

Question 32

Electron affinity

Answer 32

A neutral atom’s likelihood of gaining an electron

Question 33

What happens to electron affinity moving down a column?

Answer 33

It decreases

Question 34

What happens to electron affinity moving across a period?

Answer 34

It increases

Question 35

Electronegativity

Answer 35

Likelihood of an atom to attract a bonding pair of electrons

Question 36

What happens to electronegativity moving down a column?

Answer 36

It decreases because atomic size is increasing so their is less attraction to an atoms own and other atoms electrons

Question 37

What happens to electronegativity moving across a period?

Answer 37

It increases because atomic size is decreasing so there is more attraction to an atoms own and other atoms electrons

Question 38

Atomic radius

Answer 38

One half the distance between bonded nuclei

Question 39

What happens to atomic radius going down a column?

Answer 39

It increases because electrons are filled in orbitals farther from the nucleus, and attraction isn’t as strong

Question 40

What happens to atomic radius going across a period?

Answer 40

It decreases because electrons are being filled into the same orbitals, but there are more protons and electrons total, making there more attraction in a smaller size

Question 41

Ionic radius

Answer 41

The radius of an ion

Question 42

Ionic radius of metals

Answer 42

Less than that of a neutral atom, as metals tend to form cations that leave more protons and more attraction in the ion

Question 43

Ionic radius of non-metals

Answer 43

Greater than that of a neutral atom, as non-metals tend to form anions that leave more electrons and less attraction in the ion