2nd Six Weeks

Question 0

Pauli Exclusion principle

Answer 0

The Pauli Exclusion Principle states that, in an atom, no two electrons can have the same four electronic quantum numbers. We are aware that in one orbital a maximum of two electrons can be found and the two electrons must have opposing spins.

Question 1

Aufbau principle

Answer 1

The Aufbau principle (from the German Aufbau meaning “building up, construction”: also Aufbau rule or building-up principle) is used to determine the electron configuration of an atom, molecule or ion.

Question 2

Hund’s Rule

Answer 2

Hund’s Rule states that: Every orbital in a sublevel is singly occupied before any orbital is doubly occupied. All of the electrons in singly occupied orbitals have the same spin (to maximize total spin).

Question 3

Isotope

Answer 3

each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical properties; in particular, a radioactive form of an element.

Question 4

What are the charges of the following:
Protons
Neutrons
Electrons

Answer 4

Positive
No charge
Negative

Question 5

Atomic mass a.k.a. atomic weight, average atomic mass, & relative atomic mass

Answer 5

A weighted average of the masses for all the isotopes of a certain element

Question 6

Alpha Radiation

Answer 6

Emits alpha particles. An alpha particle is made up of two protons and two neutrons. Often called a helium nucleus

Question 7

Beta Radiation

Answer 7

Consists of fast moving electrons called beta particles (negatively charged particles)

Question 8

Gamma radiation

Answer 8

Gamma rays are high-energy radiation that possess no mass. Gamma rays usually accompany alpha and beta radiation, they account for the most energy lost during the radioactive decay process. (No mass & no charge)

Question 9

What is another word for decay?

Answer 9

Emission

Question 10

What is the name for K-capture?

Answer 10

Electron capture

Question 11

Atomic number (Z)

Answer 11

Number of protons

Question 12

Mass number (A)

Answer 12

Number of protons + neutrons

Question 13

Net charge

Answer 13

How protons and electrons balance out
Net charge = 0: neutral
Net charge = +1: ion (any item that has a net charge, even negative)

Question 14

Average atomic mass practice problem

Answer 14

Gallium-69 (60.11% abundance) 68.926 amu
Gallium-71 (39.89% abundance) 70.925 amu
68.9250.6011 + 70.9250.3989 = 69.72 amu

Question 15

Alkali Metals

Answer 15

The alkali metals are a group (column) in the periodic table consisting of the chemical elements lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr). This group lies in the s-block of the periodic table as all alkali metals have their outermost electron in an s-orbital: this electron configuration results in their characteristic properties. The alkali metals provide the best example of group trends in properties in the periodic table, with elements exhibiting well-characterized homologous behaviour.

Question 16

Alkaline earth metals

Answer 16

The alkaline earth metals are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).[4] This group lies in the s-block of the periodic table as all alkaline earth metals have their outermost electron in an s-orbital.

Question 17

Transition metals

Answer 17

The 38 elements in groups 3 through 12 of the periodic table are called “transition metals”. As with all metals, the transition elements are both ductile and malleable, and conduct electricity and heat. The interesting thing about transition metals is that their valence electrons, or the electrons they use to combine with other elements, are present in more than one shell. This is the reason why they often exhibit several common oxidation states. There are three noteworthy elements in the transition metals family. These elements are iron, cobalt, and nickel, and they are the only elements known to produce a magnetic field.

The Transition Metals are:

Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Yttrium
Zirconium
Niobium
Molybdenum
Technetium
Ruthenium
Rhodium
Palladium
Silver

Cadmium
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
Ununnilium
Unununium
Ununbium

Question 18

Non metals

Answer 18

The non-metal elements within the periodic table are:

Argon
Astatine
Bromine
Carbon
Chlorine
Fluorine
Helium
Hydrogen
Iodine
Krypton
Neon
Nitrogen
Oxygen
Phosphorus
Radon
Selenium
Sulfur
Xenon

Non-metals are either liquid or gas at room temperature, they have low electrical conductivity and have high melting and boiling points. Non-metals oxides are acidic.

Question 19

Noble Gases

Answer 19

The six noble gases are found in group 18 of the periodic table. These elements were considered to be inert gases until the 1960’s, because their oxidation number of 0 prevents the noble gases from forming compounds readily. All noble gases have the maximum number of electrons possible in their outer shell (2 for Helium, 8 for all others), making them stable.

Helium
Neon
Argon
Krypton
Xenon
Radon

Question 20

Halogens

Answer 20

The halogens are five non-metallic elements found in group 17 of the periodic table. The term "halogen" means "salt-former" and compounds containing halogens are called "salts". All halogens have 7 electrons in their outer shells, giving them an oxidation number of -1. The halogens exist, at room temperature, in all three states of matter:
Solid- Iodine, Astatine
Liquid- Bromine
Gas- Fluorine, Chlorine
The Halogens are:
Fluorine
Chlorine
Bromine
Iodine
Astatine