GenChem2 (PeriodicTable)

Question 1

Periodic Law states that the chemical properties of the elements are dependent, in a systematic way, upon their

Answer 1

Atomic numbers

Question 2

How many periods (rows) are there?

Answer 2

7

They represent n=1 to n=7

Question 3

Groups represent elements that have the same electronic configuration in their _____, and the have similar chemical properties because of it

Answer 3

Valence Shell

Question 4

The Roman numeral above each group represents the number of

Answer 4

Valence Electrons

Question 5

A groups have ____ sublevels as their outermost orbitals

B groups have _____ sublevels as their outermost orbitals

Answer 5

s and p

d and f

Question 6

The B elements include these groups

Answer 6

transition elements
lanthanide series
actinide series

Question 7

This B element group has partially filled d levels

Answer 7

Transition elements

Question 8

This B element has partially filled f sublevels

Answer 8

Lanthanide and Actinide Series

Question 9

As one goes from left to right across a period, the electrons of the outermost shell experience INCREASING/DECREASING amount of nuclear attraction

Answer 9

As one goes from left to right across a period, the electrons of the outermost shell experience INCREASING amount of nuclear attraction
(they become closer and more tightly bound to the nucleus)

Question 10

As one goes down a column, the outermost electrons become MORE/LESS tightly bound to the nucleus

Answer 10

As one goes down a column, the outermost electrons become LESS tightly bound to the nucleus

Question 11

The _____ is equal to one-half the distance between the centers of two atoms of that element that are just touching each other

Answer 11

Atomic radius

Question 12

Atomic radius ______ from right to left and ________ down a given group

Answer 12

Atomic radius decreases from right to left and increases down a given group

Question 13

The atoms with the largest atomic radius will be located where on the periodic table?

Answer 13

Bottom of group 1

Question 14

The energy required to completely remove an electron from a gaseous atom or ion.

Answer 14

Ionization Energy (IE) or Ionization Potential

Question 15

Is removing an electron exothermic or endothermic?

Answer 15

Endothermic, as it requires energy.

Question 16

The energy required to remove one valence electron from the parent atom

The energy required to remove a second valence electron from the univalent ion to form the divalent ion

Answer 16

Second Ionization energy

Question 17

Which has a greater ionization energy, second or first ionization energy?

Answer 17

second ionization energy

IEs grow increasingly large

Question 18

From left to right across the periodic table, ionization energy INCREASES/DECREASES

Why?

Answer 18

From left to right across the periodic table, ionization energy INCREASES

The atomic radius DECREASES

Question 19

Moving down a group, ionization energy INCREASES/DECREASES

Why?

Answer 19

Moving down a group, ionization energy DECREASES

The atomic radius increases

Question 20

Defined as the energy change that occurs when an electron is added to a gaseous atom, and represents the ease to with which the atom can accept an electron.

Answer 20

Electron Affinity

Question 21

Positive electron affinity (in this text) represents energy absorption when an electron is added or energy release?

Answer 21

Energy release

Question 22

Group IIA elements have HIGH/LOW electron affinityies

Group VIIA elements have HIGH/LOW electron affinities

Answer 22

Group IIA elements have LOW electron affinityies

Group VIIA elements have HIGH electron affinities

Question 23

A measure of the attraction an atom has for electrons in a chemical bond

Answer 23

Electronegativity

Question 24

Electronegativities are related to…

Answer 24

Ionization energies

Question 25

Electrons with low ionization energies have HIGH/LOW electronegativities Why?

Answer 25

Electrons with low ionization energies have LOW electronegativities Their nuclei do not strongly attract electrons.

Question 26

Electrons with high ionization energies have HIGH/LOW electronegativities Why?

Answer 26

Electrons with high ionization energies have HIGH electronegativities The nucleus has a strong pull on the electrons

Question 27

As you move from left to right across the periodic table, electronegativity ______ As you increases the atomic number in a group, electronegativity ______

Answer 27

Increases Decreases because of increased distance between valence shell and nucleus

Question 28

The three categories of elements in the periodic table

Answer 28

Nonmetals, Metals, Metalloids

Question 29

Category of elements that have high densities and high melting points, and are solid at room temperature

Answer 29

Metals

Question 30

Metalshave the ability to be deformed without breaking, like hammering it into different shapes. This characteristic ability of metals is called

Answer 30

Malleability

Question 31

The ability of metal to be drawn into a wire

Answer 31

Ductility

Question 32

Metals have a SMALL/LARGE atomic radius Metals have a HIGH/LOW IE Metals have a HIGH/LOW electronegativity These properties are explained by

Answer 32

Metals have a LARGE atomic radius Metals have a LOW IE Metals have a LOW electronegativity These properties are explained by the few electrons in the valence shell which can be easily removed.

Question 33

Metals are BAD/GOOD conductors of electricity and heat? Why?

Answer 33

Metals are GOOD conductors of electricity and heat The valence electrons can move freely

Question 34

Which metals are the most reactive metals?

Answer 34

Groups IA and IIA

Question 35

This category of elements is brittle in the solid state and show little or no metallic luster.

Answer 35

Nonmetals

Question 36

Nonmetals have HIGH/LOW IE Nonmetals have HIGH/LOW electronegativit Nonmetals are GOOD/POOR conductors of heat and electricity

Answer 36

Nonmetals have HIGH ionization energies Nonmetals have HIGH electronegativity Nonmetals are POOR conductors of heat and electricity (usually)

Question 37

Name the one characteristic of nonmetals that they share, otherwise they have a wide range of chemical behaviors and reactivities

Answer 37

Nonmetals share the ability to gain electrons easily

Question 38

The category of elements located along the line between the metals and nonmetals on the periodic table

Answer 38

Metalloids

Question 39

Are metalloid properties universal or diverse?

Answer 39

Their properties vary considerably | Densities, BPs, and MPs

Question 40

Metalloids have HIGH/LOW/INTERMEDIATE electronegativites and IEs

Answer 40

Intermediate between metals and nonmetals, they possess characteristics of both classes

Question 41

What does the reactivity of metalloids depend pon?

Answer 41

The element with which they are reacting

Question 42

B behaves as a nonmetal when reacting with... | B behaves as a metal when reacting with...

Answer 42

Na | F

Question 43

Name the elements classified as metalloids

Answer 43

Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium

Question 44

The elements of group IA are referred to as

Answer 44

Alkali Metals

Question 45

How do alkali differ from other metals? Why?

Answer 45

They have lower densities. They have one loosely bound electron in the valence shell, meaning they have the largest atomic radii in a period.

Question 46

Alkali metals have ____ IEs Alkali metals have ____ electronegativity Alkali metals have _____ reactivity Why?

Answer 46

Low IEs Low electronegativity High reactivity They easily lose their valence electron

Question 47

What group do alkali metals react easily with? Especially...

Answer 47

Nonmetals, especially halogens

Question 48

The elements of group IIA are the...

Answer 48

Alkaline earth metals

Question 49

Alkaine earths have a LARGER/SMALLER atomic radius than alkali metals

Answer 49

Smaller.

Question 50

Can the two valence electrons of alkaline earths be removed to form divalent cations?

Answer 50

Yes.

Question 51

Alkaline earths have _____ IEs | Alkaline earths have _____ electron affinities

Answer 51

Alkaline earths have LOW IEs | Alkaline earths have LOW electron affinities

Question 52

Elements in group VIIA are the...

Answer 52

Halogens

Question 53

Halogens have ____ reactivity Why?

Answer 53

Halogens have HIGH reactivity Seven electrons in the valence shell

Question 54

In terms of physical properties, are the halogens uniform or diverse?

Answer 54

Halogens are highly variable. F2 and CL2 are gaseous, Br2 is liquid, I2 is solid at room temperature

Question 55

Are the chemical properties of halogens uniform or diverse? What group of elements are halogens most reactive with?

Answer 55

Uniform. High electronegativities, high ionization energies Alkali Metals and Alkaline Earth metals (group IA and IIA)

Question 56

The group of elements found in group VIIIA are the...

Answer 56

Noble Gases

Question 57

The noble gases are REACTIVE/NONREACTIVE The noble gases have HIGH/LOW IEs The noble gases have HIGH/LOW electronegativities Why?

Answer 57

NONREACTIVE HIGH IEs NO ELECTRONEGATIVITIES Noble gases have a full valence shull

Question 58

Groups IB to VIIIB are the

Answer 58

Transition metals.

Question 59

The transition metals are very SOFT/HARD The transition metals have HIGH/LOW melting points Transition elements have HIGH/LOW IEs

Answer 59

The transition metals are very HARD The transition metals have HIGH BPs The transition metals have LOW IEs

Question 60

Transition metals may exist in a variety of positively charged forms, aka Why?

Answer 60

Oxidation states Transition metals are capable of losing various numbers of electrons from the s and d orbitals of the valence shell

Question 61

Dissolves ions of transition metals can form ____ with other molecules of water or with nonmetals Does the formation of complex ions increase or decrease the solubility of a compound?

Answer 61

Complex Ions It enhances the solubility

Question 62

What gives the complex ions their characteristic colors?

Answer 62

The d orbitals split into two energy sublevels, enabling complexes to absorb certain frequencies of light. Those not absorbed are observed.