The Periodic Table

Question 1

The modern periodic table is organized based on increasing _____ _____.

Answer 1

Atomic number

Question 2

Rows of elements on the periodic table are referred to as ______; columns are called ______.

Answer 2

Periods; groups (or families)

Question 3

The A elements are known as the _______ elements and include groups IA through VIIIA. The elements in these groups have their valence electrons in the orbitals of either s or p subshells.

Answer 3

Representative

Question 4

The B elements are known as the ________ elements and include both the transition elements, which have valence electrons in the s and d subshells, and the lanthanide and actinide series, which have valence electrons in the s and f subshells.

Answer 4

Nonrepresentative

Question 5

Metals are found on the left side and in the middle of the periodic table. List some characteristics of metals.

Answer 5

1. Lustrous (shiny) solids (except for Hg at room temp.)
2. Generally, high melting points and densities
3. Malleable
4. Ductile
5. Good conductors of heat and electricity (due to their electrons being free to move)

Question 6

True or false: Metals easily give up electrons, which leads to characteristics such as low ionization energy and low electron affinity.

Answer 6

True

Question 7

Nonmetals are found on the upper right side of the periodic table. What are some characteristics of nonmetals?

Answer 7

1. Brittle and show little or no metallic luster
2. High ionization energies, electron affinities, and electronegativities
3. Poor conductors of heat and electricity
   (All of these characteristics are manifestations of the inability of nonmetals to easily give up electrons.)

Question 8

(HIGH YIELD) The electrostatic attraction between the valence shell electrons and the nucleus is known as the _____ _____ _____, a measure of the net positive charge experienced by the outermost electrons.

Answer 8

Effective nuclear charge (Z sub eff)

Question 9

(HIGH YIELD) For elements in the same period, does the effective nuclear charge increase or decrease from left to right?

Answer 9

Increase

Question 10

(HIGH YIELD) From top to bottom in a group, does the effective nuclear charge increase or decrease, or is it held constant?

Answer 10

It is held constant because the increased shielding created by the inner shell electrons cancels the increased positivity of the nucleus.

Question 11

(HIGH YIELD) The _____ _____ of an atom is equal to half the distance between the centers of two atoms of an element that are briefly in contact with each other.

Answer 11

Atomic radius

Question 12

(HIGH YIELD) Describe how atomic radii change as you move across and down the periodic table.

Answer 12

Atomic radii decrease as you move from left to right across a period; they increase as you move from top to bottom down a group.

Question 13

(HIGH YIELD) _______ _______ is the energy required to remove an electron from a gaseous species.

Answer 13

Ionization energy (IE)

Question 14

(HIGH YIELD) Is the removal of an electron from an atom an exothermic or endothermic process?

Answer 14

Endothermic

Question 15

(HIGH YIELD) Describe how ionization energy changes as you move across and down the periodic table.

Answer 15

Ionization energy increases from left to right and decreases from top to bottom (because the electrons are held less tightly by the nucleus as the principal quantum number increases).

Question 16

(HIGH YIELD) True or false: The second ionization energy is always greater than the first ionization energy.

Answer 16

True. Electrons are being removed from increasingly cationic (positive) species.

Question 17

(HIGH YIELD) The active metals are found in what groups?

Answer 17

Groups IA and IIA (Groups 1 and 2)

Question 18

(HIGH YIELD) Which group of elements is the least likely to give up electrons?

Answer 18

Group VIIIA (Group 18) elements, or the Noble gases. They are among the elements with the highest ionization energies.

Question 19

(HIGH YIELD) When an atom acquires an electron, is this an endothermic or exothermic process?

Answer 19

Exothermic

Question 20

(HIGH YIELD) Describe how electron affinity changes as you move across and down the periodic table.

Answer 20

Electron affinity increases from left to right and decreases from top to bottom.

Question 21

(HIGH YIELD) ________ is a measure of the attractive force than an atom will exert on an electron in a chemical bond.

Answer 21

Electronegativity. It increases from left to right and decreases from top to bottom.

Question 22

List the common names for each of the following groups on the periodic table: Group 1, Group 2, Group 16, Group 17, Group 18, and Groups 3-12

Answer 22

Group 1 - Alkali Metals
Group 2 - Alkaline Earth Metals
Group 16 - Chalcogens
Group 17 - Halogens
Group 18 - Noble Gases
Groups 3 - 12: Transition Metals

Question 23

One of the unique properties of the transition metals is that many of them can have different possible charged forms or ______ ______ because they are capable of losing different numbers of electrons from the s- and d-orbitals in their valence shells.

Answer 23

Oxidation states

Question 24

Antimony is used in some antiparasitic medications. What type of element is antimony (Sb)?

Answer 24

Metalloid

Question 25

Which property of metals explains why they are used in making wires that conduct electricity?

Answer 25

Metals have valence electrons that can move freely.