Chapter 2: The Periodic Table Flashcards

1
Q

The periodic table is organized based on increasing atomic ________.

A

number

the # of protons in an element

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2
Q

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 ________.

A

their atomic numbers

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3
Q

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

A

valence shell

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4
Q

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.

A

valence electrons; greatest

held less tightly by the nucleus; can mingle

largest determinant of chemical reactivity

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5
Q

The Roman numeral above each group represents what?

A

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

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6
Q

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

A

representative; s or p subshells

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7
Q

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?

A

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

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8
Q

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

A

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

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9
Q

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

A

malleable; ductile

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10
Q

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.

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

allow metals to easily give up electrons

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11
Q

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

A

oxidation states

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12
Q

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

A

conductors

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13
Q

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.

A

s; s and d; s and f

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14
Q

____________ 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.

A

Nonmetals; brittle

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15
Q

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.

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

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

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16
Q

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.

A

metalloids

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

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17
Q

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

A

effective nuclear charge

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18
Q

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

A

increases; adding a proton

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19
Q

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

A

octet

there are exceptions!

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20
Q

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

A

atomic radius

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21
Q

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

A

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

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22
Q

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

A

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

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23
Q

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

A

ionic radius

24
Q

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.

A

gain; larger

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.
lose
26
____________ ________ is the energy required to remove highest energy electrons
ionization energy
27
Ionization energy is an ________________ process, as it requires input of heat
endothermic
28
The energy to remove the first e- is called the ________ IE.
first
29
An atom whose first valence e- has been removed is called a ________ cation (X+) and forms a divalent cation.
univalent
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.
active
31
The halogens (Group 17) typically (lose/gain?) an electron and are generally (cations/anions?).
gain; anions
32
A halogen gaining an electron to complete its octet is an ____________ process because it expels energy in the form of heat.
exothermic
33
________ ________ refers to the energy dissipated by a gaseous species when it gains an electron.
Electron affinity | essentially opposite from IE
34
Since electron affinity (gaining) is an exothermic process, ΔHrxn has a (negative/positive?) sign. However, electron affinity is reported as a (negative/positive?) number
negative; positive
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.
greater
36
Electron affinity (increases/decreases?) from left to right. Why?
Increases, because Zeff increases
37
Eleectron affinity (increases/decreases?) top to bottom, why?
decreases, because the valence shells are farther away
38
____________________ is the measure of attractive force that an atom exerts on an electron in a bond.
Electronegativity
39
Electronegativity is related to ________________ ________.
ionization energy
40
The lower the ionization energy, the (lower/higher?) the electronegativity is.
lower
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.
alkali; 1
42
The alkali metals have very (low/high?) Zeff, and thus have the (largest/smallest?) atomic radii of all the elements.
low; largest
43
Alkali metals react readily with ____________, especially which group?
nonmetals; halogens
44
The ____________ ________ ________ have many properties of the alkali metals but have slightly (lower/higher?) Zeff and thus slightly (smaller/larger?) atomic radii.
alkaline earth metals; higher; smaller
45
The alkali metals usually form ________ cations.
univalent
46
The alkaline earth metals usually form ________ cations.
divalent
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.
chalcogens; 16 small; large | most important are oxygen, sulfur, and selenium; the rest are metals
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.
halogens, 17
49
Halogens are so reactive that they are not naturally found in their elemental state but rather as ions called ________ or as ________ molecules.
halides; diatomic
50
The ________ gases have extremely low boiling points and exist as gases at RT.
noble
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.
transition; 3 to 12
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.
oxidation states | causes many different ionic compounds to form
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.
hydration complexes
54
The ability to form hydration complexes contributes to the variable ________________ of certain transition metal-containing compounds.
solubility ## Footnote e.g. AgCl can dissolve in ammonia but not water bc it forms a complex w/ it
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.
d ## Footnote The frequencies not absorbed (subtraction frequencies), give complexes their color
56
When we perceive an object as a particular color, it is because that color is not absorbed, but rather ____________ by the object.
reflected
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.
subtraction frequencies; complementary color