Periodic Properties of the Elements

Question 1

Rows of the periodic table are referred to as _______.

Answer 1

Periods

Question 2

Columns of the periodic table are referred to as ______ or ________.

Answer 2

Groups or families

Question 3

All elements from the periodic table can be categorized into which three categories?

Answer 3

Metals, nonmetals, and metalloids

Question 4

A description of the orbitals occupied by electrons is called an ________ _____________.

Answer 4

Electron configuration

Question 5

Paired spins are ___________.

Answer 5

Diamagnetic

Question 6

What is the Pauli Exclusion Principle?

Answer 6

No two electrons in an atom may have the same set of four quantum numbers; no orbital may have more than two electrons, and the electrons must have opposite spins

Question 7

What are degenerate orbitals?

Answer 7

Orbitals with the same energy (E)

Question 8

What is the aufbau principle?

Answer 8

Electrons fill atomic orbitals from lowest energy to highest.

Question 9

What is shielding?

Answer 9

A phenomenon that reduces the attraction between an electron and the nucleus in an atom caused by the repulsion of the core electrons on the outer electrons.

Question 10

What is the effective nuclear charge (Zeff)?

Answer 10

The net positive charge that is attracting a particular electron

Question 11

What is Hund’s rule?

Answer 11

Filling orbitals that have the same energy (degenerate) place one electron in each orbital before completing pairs

Question 12

What are core (inner) electrons? What are valence electrons?

Answer 12

Electrons in lower-energy shells; electrons in all the sublevels with the highest principal energy shell

Question 13

Which electrons participate in bonding?

Answer 13

Valence electrons

Question 14

Which transition metals have irregular electron configurations? What is the anomaly in these configurations?

Answer 14

Copper (Cu), Silver (Ag), Chromium (Cr), Molybdenum (Mo); An s electron jumpts to a d orbital to create a half-filled (Cr & Mo) or completely filled (Cu & Ag) sublevel

Question 15

What aspect of electron configuration is different for transition metals (d block) and inner transition metals (f block) than main group elements? Why?

Answer 15

Because of sublevel splitting, the 4s sublevel is lower in energy than the 3d sublevel; thus, the 4s orbital fills before the 3d

Question 16

What group in the periodic table has eight valence electrons?

Answer 16

Noble gases, 8A (except for Helium, with two)

Question 17

What group in the periodic table is especially nonreactive?

Answer 17

Noble gases

Question 18

What are the four groups of metals in the periodic table?

Answer 18

Alkali metals, alkaline earth metals, transition/inner transition metals, p-block metals

Question 19

Where are metalloids located in the periodic table?

Answer 19

In the p-block area of the periodic table between the metal and nonmetal elements

Question 20

Where are nonmetals located in the periodic table?

Answer 20

The upper right-hand side, in the p-block area

Question 21

Metals form _______. Nonmetals form ______.

Answer 21

Cations (positively charged atoms), anions (negatively charged atoms)

Question 22

Describe the periodic trends for effective nuclear charge.

Answer 22

Increases across a period; decreases down a group

Question 23

What is atomic radius?

Answer 23

The average radius of an atom based on measuring large numbers of elements and compounds

Question 24

Describe the periodic trends for atomic radius.

Answer 24

Decreases across a period; increases down a group

Question 25

The larger the effective nuclear charge an electron experiences, the ________ the attraction it will have to the nucleus.

Answer 25

Stronger

Question 26

Describe the periodic trends for atomic radius (for transition elementals).

Answer 26

Increase down a group; little correlation across a period

Question 27

What is paramagnetism?

Answer 27

Atoms or ions that have a net magnetic field due to unpaired electrons in their electron configuration

Question 28

What is diamagnetism?

Answer 28

Atoms or ions that slightly repel a magnetic field due to having all paired electrons in their electron configuration

Question 29

Cation radius is _______ than its corresponding atom radius.

Answer 29

Smaller

Question 30

Anion radius is ______ than its corresponding atom radius.

Answer 30

Larger

Question 31

What does isoelectronic mean?

Answer 31

Having the same electron configuration

Question 32

Describe the periodic trends for ionic radii.

Answer 32

Increases down a group

Question 33

What is ionization energy?

Answer 33

Minimum energy needed to remove an electron from an atom

Question 34

Define endothermic and exothermic. Is removing an electron from an atom and endothermic or exothermic process?

Answer 34

Endothermic processes requires the input of energy while exothermic processes release energy; removing electrons in always an endothermic process

Question 35

Describe the periodic trend for first ionization energy.

Answer 35

Decreases down a group; increases across a period

Question 36

Removal of each successive electron costs ____ energy.

Answer 36

More

Question 37

Describe the periodic trends for electron affinity.

Answer 37

Increases across a period; little correlation down a group

Question 38

What is metallic character?

Answer 38

How closely an element’s properties match the ideal properties of a metal

Question 39

Describe the periodic trends for metallic character.

Answer 39

Decreases across a period; increases down a group

Question 40

______ generally have smaller first ionization energies and _________ generally have larger electron affinities.

Answer 40

Metals, nonmetals