MIDTERM STUDY (unit 4/5

Question 1

Only s and p orbitals are

Answer 1

Valence electrons

Question 2

Valence electrons:

Answer 2

e- in outer most energy level

Question 3

s sublevel:

Answer 3

2 e- and Sphere shape

Question 4

p sublevel:

Answer 4

6 e- and dumbbell shape

Question 5

Principles that govern electron configuration:

Answer 5

• Pauli Exclusion Principle
• Hund’s Rule
• Aufbau Principle

Question 6

Pauli Exclusion Principle:

Answer 6

2 e- in same orbital must have opp spins

Question 7

Hunds Rule:

Answer 7

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

Question 8

Aufbau principle:

Answer 8

e- occupy positions of lowest energy level first

Question 9

Orbital Notation:

Answer 9

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

Question 10

Lewis Dot Notation:

Answer 10

shows only valence e-

Question 11

Bohr Model Diagram:

Answer 11

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

Question 12

Electron Configuration:

Answer 12

use of superscripts to show the # of electrons per sublevel

Question 13

Nobel Gas Configuration:

Answer 13

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

Question 14

Isoelectronic:

Answer 14

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

Question 15

Dimitri Mendeleev:

Answer 15

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

Question 16

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

Answer 16

they were undiscovered elements

Question 17

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

Answer 17

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

Question 18

Henry Moseley:

Answer 18

ordered elements by atomic number (# of p+)

Question 19

Periodic Law:

Answer 19

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

Question 20

Periodic groups;

Answer 20

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

Question 21

Periodic Periods:

Answer 21

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

Question 22

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

Answer 22

its group # or group number minus 10

Question 23

What are the three classes of elements:

Answer 23

Metals, Nonmetals, Metalloids

Question 24

How are elements arranged:

Answer 24

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

Question 25

Properties of metals:

Answer 25

-easily oxidized (lose e-)
- good electrical conductors
-shiny, malleable, ductile
- low ionization energies
-low electronegativities

Question 26

Properties of Nonmetals:

Answer 26

-gain e- (are reduced)
-not conductors
- dull,brittle
-high ionization energies
- high electronegativity

Question 27

(4 types) Metals:

Answer 27

Alkali Metals
Alkaline Earth Metals
Transition Metals
Inner transition metals

Question 28

(2 types) NonMetals:

Answer 28

Halogens
Noble Gases

Question 29

Alkali Metals:

Answer 29

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

Question 30

Alkaline Earth Metals:

Answer 30

have 2 valence e-
less reactive
not found in pure form
“Basic”

Question 31

Transition Metals:

Answer 31

d/block elements

Question 32

Inner Transition Metals:

Answer 32

lanthanides and actinides

Question 33

(3 things) Halogens:

Answer 33

have 7 valence e-
most reactive group of NONMETALS
ONLY found in pure form as diatomic element

Question 34

(4 things ) Noble Gases:

Answer 34

8 valence e-
chemically unreactive
only found in pure form in nature
colorless and odorless

Question 35

Atomic Radius:

Answer 35

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

Question 36

Atomic Radii:

Answer 36

one half the distance between the nuclei of identical atoms that are bonded together

Question 37

Ionization energy def:

Answer 37

energy required to remove one electron from an atom

Question 38

Ionization energy:

Answer 38

-As atomic radius decreases across the period, valence e- being removed is closer to positive nucleus so harder to remove and need more energy

Question 39

Electronegativity def:

Answer 39

a measure of the ability of an atom in a chemical compound to attract e- from another atom

Question 40

Electronegativity:

Answer 40

as atomic radius decreases across period, the positive nuclear charge increases making the atom’s ability to “pull in” e- much greater

Question 41

Ionic Radius:

Answer 41

Metals- decreases
nonmetals- increases

Question 42

Metals:

Answer 42

valence e- are lost to create cations

Question 43

Nonmetals:

Answer 43

Valence e- are gained to create anions

Question 44

Period Trends:

Answer 44

(across the period) affected by increasing nuclear charge, an increasing number of p+ but same number of energy levels.

Question 45

Group Trends:

Answer 45

(down the group) affected by shielding. shielding increases down the group due to increasing # of energy levels

Question 46

Shielding:

Answer 46

inner levels of e- repel the outer (valence) e- blocking the nuclear effect on the e-

Question 47

How many naturally occurring elements are there?

Answer 47

92

Question 48

Periodic Families (groups):

Answer 48

Alkali metals
alkaline earth metals
transition metals
Halogens
Noble Gases
Lanthanides (inner transition metals)
Actinides ( inner transition metals)