MIDTERM STUDY (unit 4/5 Flashcards

1
Q

Only s and p orbitals are

A

Valence electrons

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2
Q

Valence electrons:

A

e- in outer most energy level

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3
Q

s sublevel:

A

2 e- and Sphere shape

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4
Q

p sublevel:

A

6 e- and dumbbell shape

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5
Q

Principles that govern electron configuration:

A
  • Pauli Exclusion Principle
  • Hund’s Rule
  • Aufbau Principle
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6
Q

Pauli Exclusion Principle:

A

2 e- in same orbital must have opp spins

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7
Q

Hunds Rule:

A

e- in same sublevels occupy empty orbitals before they pair up

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8
Q

Aufbau principle:

A

e- occupy positions of lowest energy level first

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9
Q

Orbital Notation:

A

shows all e- in energy level order, with e- pairing, and opp spins

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10
Q

Lewis Dot Notation:

A

shows only valence e-

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11
Q

Bohr Model Diagram:

A

shows all e- per energy level (does not delineate between sublevels)

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12
Q

Electron Configuration:

A

use of superscripts to show the # of electrons per sublevel

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13
Q

Nobel Gas Configuration:

A

use of Nobal Gas from the period above, then show configuration of e- after that noble gas

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14
Q

Isoelectronic:

A

atoms of two different elements with the same # of e-

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15
Q

Dimitri Mendeleev:

A

developed periodic table of known elements and arranged them in order of increasing atomic mass and later ordered according to chemical properties

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16
Q

What did Mendeleev predict about the empty spaces in his periodic table:

A

they were undiscovered elements

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17
Q

What was the problem with Mendeleev’s new periodic table:

A

When elements were arranged according to similar properties, some had to be placed out of order of atomic mass

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18
Q

Henry Moseley:

A

ordered elements by atomic number (# of p+)

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19
Q

Periodic Law:

A

states that the physical and chemical properties of elements are periodic functions of their atomic #’s

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20
Q

Periodic groups;

A

(18) Elements of the same group have same valence configuration, valence electrons, and similar chemical properties

21
Q

Periodic Periods:

A

(7) elements of same period have the sma e# of occupied energy levels

22
Q

The number of valence electrons in MAIN GROUP ELEMENTS is = to

A

its group # or group number minus 10

23
Q

What are the three classes of elements:

A

Metals, Nonmetals, Metalloids

24
Q

How are elements arranged:

A

in order of increasing atomic # (# of protons) NOT MASS

25
Properties of metals:
-easily oxidized (lose e-) - good electrical conductors -shiny, malleable, ductile - low ionization energies -low electronegativities
26
Properties of Nonmetals:
-gain e- (are reduced) -not conductors - dull,brittle -high ionization energies - high electronegativity
27
(4 types) Metals:
Alkali Metals Alkaline Earth Metals Transition Metals Inner transition metals
28
(2 types) NonMetals:
Halogens Noble Gases
29
Alkali Metals:
have 1 valence e- NEVER found in pure form bc too reactive Reactivity increases down group Most reactive group of metals soft and silvery in color
30
Alkaline Earth Metals:
have 2 valence e- less reactive not found in pure form "Basic"
31
Transition Metals:
d/block elements
32
Inner Transition Metals:
lanthanides and actinides
33
(3 things) Halogens:
have 7 valence e- most reactive group of NONMETALS ONLY found in pure form as diatomic element
34
(4 things ) Noble Gases:
8 valence e- chemically unreactive only found in pure form in nature colorless and odorless
35
Atomic Radius:
Left to right # of energy levels stay the same and # of protons increases in nucleus so it increases the positive nuclear charge - pulls the electrons in closer
36
Atomic Radii:
one half the distance between the nuclei of identical atoms that are bonded together
37
Ionization energy def:
energy required to remove one electron from an atom
38
Ionization energy:
-As atomic radius decreases across the period, valence e- being removed is closer to positive nucleus so harder to remove and need more energy
39
Electronegativity def:
a measure of the ability of an atom in a chemical compound to attract e- from another atom
40
Electronegativity:
as atomic radius decreases across period, the positive nuclear charge increases making the atom's ability to "pull in" e- much greater
41
Ionic Radius:
Metals- decreases nonmetals- increases
42
Metals:
valence e- are lost to create cations
43
Nonmetals:
Valence e- are gained to create anions
44
Period Trends:
(across the period) affected by increasing nuclear charge, an increasing number of p+ but same number of energy levels.
45
Group Trends:
(down the group) affected by shielding. shielding increases down the group due to increasing # of energy levels
46
Shielding:
inner levels of e- repel the outer (valence) e- blocking the nuclear effect on the e-
47
How many naturally occurring elements are there?
92
48
Periodic Families (groups):
Alkali metals alkaline earth metals transition metals Halogens Noble Gases Lanthanides (inner transition metals) Actinides ( inner transition metals)