Chapter 2: The Periodic Table

Question 1

The periodic table is organized based on increasing atomic ________.

Answer 1

number

the # of protons in an element

Question 2

The periodic table is a visual representation of the periodic law, which states: the chemical and physical properties of the elements are dependent, in a periodic way, upon ________.

Answer 2

their atomic numbers

Question 3

Groups contain elements that have the same electronic configuration in their ________ ________ and share similar chemical properties.

Answer 3

valence shell

Question 4

The electrons in the valence shell, known as the ________ ________, are the farthest away from the nucleus and have the (greatest/least?) amount of potential energy.

Answer 4

valence electrons; greatest

held less tightly by the nucleus; can mingle

largest determinant of chemical reactivity

Question 5

The Roman numeral above each group represents what?

Answer 5

The # of valence electrons that elements in that group have in their neutral state

also has an A or B to separate the elements into 2 larger classes

Question 6

The A elements are known as the ________________ elements and they have their valence electrons in which orbitals?

Answer 6

representative; s or p subshells

Question 7

The B elements are known as the ____________________ elements and include both the ________________ elements, which have valence electrons in which subshells?

They also include the ________________ and ________________ series, which have valence electrons in which subshells?

Answer 7

nonrepresentative; transition, s and d; lanthanide and actinide, s and f

Question 8

________ are found on the left side and in the middle of the table. What 4 types do they include?

Answer 8

Metals;
1. Active
2. Transition
3. Lanthanide
4. Actinide

Question 9

Metals are ________, meaning they can be hammered into shapes. They are also ________, meaning they can be pulled or drawn into wires.

Answer 9

malleable; ductile

Question 10

Metals have:
1. (high/low?) effective nuclear charge
2. (high/low?) electronegativity
3. (small/large?) atomic radius
4. (small/large?) ionic radius
5. (high/low?) ionization energy
6. (high/low?) electron affinity.

Answer 10

1. low
2. low
3. large
4. small
5. low
6. low

allow metals to easily give up electrons

Question 11

Many transition metals (Group B) elements have 2+ ________________ ________, which are charges when forming bonds with other atoms.

Answer 11

oxidation states

Question 12

Valence electrons of metals are loosely held onto and are thus free to move, which makes metals good ________________ of electricity and heat.

Answer 12

conductors

Question 13

Valence electrons of the active metals are found in the ____ subshell; those of the transition metals are found in the ____ and ____ subshells; and those of the lanthanide and actinide series elements are in the ____ and ____ subshells.

Answer 13

s; s and d; s and f

Question 14

____________ are found predominantly on the upper right side of the periodic table. They are ____________ (texture) in the solid state and are not very lustrous, if at all.

Answer 14

Nonmetals; brittle

Question 15

Nonmetals have:
1. (high/low?) ionization energy
2. (high/low?) electron affinity
3. (high/low?) electronegativity
4. (small/large?) atomic radii
5. (small/large?) ionic radii

They are not good conductors.

Answer 15

1. high
2. high
3. high
4. small
5. large

do not easily give up e-‘s; less unified in chemical/physical properties

Question 16

Separating the metals and nonmetals are a stair-step group of elements called the ________________, also known as semimetals. The electronegativities and ionization energies of the metalloids are inbetween metals and nonmetals.

Answer 16

metalloids

boron, silicon, germanium, arsenic, antimony, tellurium, polonium, astatine

Question 17

The electrostatic attraction between the valence shell electrons and nucleus is known as ____________ ____________ ____________ - measure of net positive charge experienced by the outermost eleectrons.

Answer 17

effective nuclear charge

Question 18

Z_{eff (decreases/increases?) from left to right. Why?}

Answer 18

increases; adding a proton

Question 19

Elements can gain/lose electrons in order to achieve a stable ____________, representative of the noble (inert) gas.

Answer 19

octet

there are exceptions!

Question 20

________ ________ is 1/2 the distance between centers of 2 atoms of an element

Answer 20

atomic radius

Question 21

Atomic radius (increases/decreases?) from left to right. Why?

Answer 21

decreases; electrons are added to the outermost shell with no additional shielding; increased positive charge means increased Zeff

Question 22

Atomic radius (increases/decreases?) going down a group. Why?

Answer 22

increases; valence electrons are farther away with a virtually constant Zeff

Question 23

________ ________ is the radius of a monatomic ion in an ionic crystal structure

Answer 23

ionic radius

Question 24

For nonmetals close to the metalloid line, they need to (gain/lose?) more e- to achieve an octet, and thus have a (smaller/larger?) ionic radius.

Answer 24

gain; larger

Question 25

For metals close to the metalloid line, they have more e- to (gain/lose?) to achieve an octet, and thus experience less drastic reduction in radius during ionization.

Answer 25

lose

Question 26

____________ ________ is the energy required to remove highest energy electrons

Answer 26

ionization energy

Question 27

Ionization energy is an ________________ process, as it requires input of heat

Answer 27

endothermic

Question 28

The energy to remove the first e- is called the ________ IE.

Answer 28

first

Question 29

An atom whose first valence e- has been removed is called a ________ cation (X^{+) and forms a divalent cation.}

Answer 29

univalent

Question 30

Elements in Groups 1 and 2 have such low ionization energies that they are called ________ metals. They do not exist in their neutral forms and are always found as ionic compounds.

Answer 30

active

Question 31

The halogens (Group 17) typically (lose/gain?) an electron and are generally (cations/anions?).

Answer 31

gain; anions

Question 32

A halogen gaining an electron to complete its octet is an ____________ process because it expels energy in the form of heat.

Answer 32

exothermic

Question 33

________ ________ refers to the energy dissipated by a gaseous species when it gains an electron.

Answer 33

Electron affinity

essentially opposite from IE

Question 34

Since electron affinity (gaining) is an exothermic process, ΔH_{rxn has a (negative/positive?) sign. However, electron affinity is reported as a (negative/positive?) number}

Answer 34

negative; positive

Question 35

The stronger the electrostatic pull between nucleus and VE is, the (greater/lesser?) the energy release will be when an atom gains an electron.

Answer 35

greater

Question 36

Electron affinity (increases/decreases?) from left to right. Why?

Answer 36

Increases, because Zeff increases

Question 37

Eleectron affinity (increases/decreases?) top to bottom, why?

Answer 37

decreases, because the valence shells are farther away

Question 38

____________________ is the measure of attractive force that an atom exerts on an electron in a bond.

Answer 38

Electronegativity

Question 39

Electronegativity is related to ________________ ________.

Answer 39

ionization energy

Question 40

The lower the ionization energy, the (lower/higher?) the electronegativity is.

Answer 40

lower

Question 41

The ________ metals (Group ____) possess most of the classic physical properties of metals, except that their densities are lower than those of other metals. They only have 1 loosely bound electron in their outermost shells.

Answer 41

alkali; 1

Question 42

The alkali metals have very (low/high?) Zeff, and thus have the (largest/smallest?) atomic radii of all the elements.

Answer 42

low; largest

Question 43

Alkali metals react readily with ____________, especially which group?

Answer 43

nonmetals; halogens

Question 44

The ____________ ________ ________ have many properties of the alkali metals but have slightly (lower/higher?) Zeff and thus slightly (smaller/larger?) atomic radii.

Answer 44

alkaline earth metals; higher; smaller

Question 45

The alkali metals usually form ________ cations.

Answer 45

univalent

Question 46

The alkaline earth metals usually form ________ cations.

Answer 46

divalent

Question 47

The ____________, which are Group ____, are a group of nonmetals and metalloids. They are not as reactive as halogens, but are crucial for normal biological functions. They each have 6 electrons in their valence shell and have (small/large?) atomic radii and (small/large?) ionic radii.

Answer 47

chalcogens; 16
small; large

most important are oxygen, sulfur, and selenium; the rest are metals

Question 48

The ________, Group ____, are highly reactive nonmetals with 7 valenc e-. They have variabel physical properties and are desperate to complete their octet. VERY reactive with alkali and alkaline earth metals.

Answer 48

halogens, 17

Question 49

Halogens are so reactive that they are not naturally found in their elemental state but rather as ions called ________ or as ________ molecules.

Answer 49

halides; diatomic

Question 50

The ________ gases have extremely low boiling points and exist as gases at RT.

Answer 50

noble

Question 51

The ____________ metals (Groups ____ to ____) are considered metals and have (high/low?) electron affinities, (high/low?) ionization energies, and (high/low?) electronegativities. They are hard and have high metling and boiling points. They tend to be malleable and good conductors since they have loosely held electrons that fill the d-orbitals.

Answer 51

transition; 3 to 12

Question 52

Transition metals have different possible charged forms or ____________ ________ because they can lose different numbers of e- from the s and d orbitals in their valence shells.

Answer 52

oxidation states

causes many different ionic compounds to form

Question 53

Metals in different oxidation states form complex ions that tend to associate in solution either with molecules of water and form ________________ ________ or with nonmetals.

Answer 53

hydration complexes

Question 54

The ability to form hydration complexes contributes to the variable ________________ of certain transition metal-containing compounds.

Answer 54

solubility

e.g. AgCl can dissolve in ammonia but not water bc it forms a complex w/ it

Question 55

The formation of complexes causes the ____-orbital to split into 2 energy sublevels This enables many complexes to absorb certain frequencies of light– those containing the precise amount of energy required to raise e- from the lower to higher energy d-orbitals.

Answer 55

d

The frequencies not absorbed (subtraction frequencies), give complexes their color

Question 56

When we perceive an object as a particular color, it is because that color is not absorbed, but rather ____________ by the object.

Answer 56

reflected

Question 57

If an object absorbs a given color of light and reflects all others, our brain mixes these ________________ ________________ and we perceive the ____________________ ________ of the frequency that was absorbed.

Answer 57

subtraction frequencies; complementary color