Unit 4: The Quantum Model of the Atom and Periodic Properties

Question 1

The Heisenburg Uncertainty Principle

Answer 1

You cannot determine both the speed and the location of a particular electron at the same time.

Question 2

DeBroglie

Answer 2

Using Bohr’s model of the atom, he investigated the photoelectric effect and determined that electrons had wave-like behavior along with particle behavior, and this wave-like behavior gave them a certain frequency.

Question 3

Photoelectric Effect

Answer 3

the energy given off when light strikes metal

Question 4

Erwin Schrodinger

Answer 4

developed an equation that treated electrons in atoms as waves and this, along with Heisenburg’s research, laid the foundation to the Quantum Theory

Question 5

Max Planck

Answer 5

suggested that hot objects emit energy in small, specific amounts called Quanta

Question 6

Albert Einstein

Answer 6

capitalized on Planck’s suggestion with the idea that electromagnetic radiation had wavelike properties, that particles will “stream” and that each particle of light carries a certain quantum of energy

Question 7

Quantum Theory

Answer 7

gives us a mathematical description of the wave properties of electrons and other very small particles

Question 8

Principle Quantum Number

Answer 8

indicates the size of the atom and is symbolized using the letter “n”. “n” can be determined by locating the row the element is on as placed on the periodic table

Question 9

Azimuthal/Angular Momentum Quantum Number

Answer 9

indicates the sub levels of the main energy levels and is symbolized by the letter “l”. Also symbolized by the letters “s”, “p”, “d”, “f”, “g”, etc.

Question 10

Magnetic Quantum Number

Answer 10

indicates the orientation of the electrons on an “x”, “y”, “z” axis and is symbolized by the letter “m”.

Question 11

Spin Quantum Number

Answer 11

indicates the direction in which the electrons are traveling, +1/2 or -1/2 or by using alternating arrows.

Question 12

Hund’s Rule

Answer 12

electrons will remain unpaired as long as possible, because they have the same charge, and that like-charge will cause repulsion and excess energy. When filling sub levels, electrons will alternate spaces to put as much distance between each other before pairing

Question 13

Electron Configuration Notation (ECN)

Answer 13

a shorthand method used to write the electron configuration of elements

Question 14

Shorthand ECN

Answer 14

uses noble gas to represent sub levels that are perfectly filled

Question 15

Valence

Answer 15

electrons found in the last main level of an atom

Question 16

Ionic Bonds

Answer 16

will form between metals (cations) and nonmetals (anions) and produce compounds with high melting points that are also hard and brittle. This forms by a transfer of valence electrons.

Question 17

Covalent Bonds

Answer 17

form when valence electrons are shared between two or more atoms, usually nonmetals

Question 18

Dmitri Mendeleev

Answer 18

published the 1st periodic table in 1869 based on increasing atomic weight. He left blanks for elements he knew were still undiscovered. He also did not have an element representative of the Noble gases, because they had not been discovered yet (they were discovered in the late 1800s, early 1900s)

Question 19

Henry Mosely

Answer 19

used x-rays to confirm Mendeleev’s periodic chart which led to the Periodic Law

Question 20

Periodic Law

Answer 20

states that the physical and chemical properties of the elements are periodic functions of their atomic numbers

Question 21

How many groups does the periodic table have?

Answer 21

18

Question 22

How many series (sometimes called periods) does the periodic table have?

Answer 22

7

Question 23

Group I of the periodic table; all of these have one valence electron, explode when placed in water; form VERY strong bases, such as sodium hydroxide

Answer 23

Alkali Metals

Question 24

Chemical Bond

Answer 24

a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

Question 25

Group II of the periodic table; all of these elements have 2 valence electrons. These elements are found in many compounds in nature such as limestone and chlorophyll

Answer 25

Alkaline Earth Metals

Question 26

Groups 3-12 of the periodic table; these elements vary in their number of valence electrons. These elements are known for their brightly colored compounds.

Answer 26

Transition Metals

Question 27

Group 17 of the periodic table; these elements have 7 valence electrons. They are the most active nonmetals. They can form very strong acids, such as HCI, hydrochloric acid-stomach acid.

Answer 27

The Halogens

Question 28

Group 18 of the periodic table; all BUT helium have 8 valence electrons. They are all gases, all perfect, all non-reactive, all inert. Helium has 2 valence electrons.

Answer 28

The Noble Gases

Question 29

Atomic Radius

Answer 29

one-half the distance between like nuclei that are bonded together. It increases as you go down a group, decreases as you move from left to right on the periodic table. Metallic characteristics decrease as you go left to right, decreases as you go from top to bottom. If energy is high, it is small.

Question 30

Ionization Energy

Answer 30

the energy required to remove valence electrons from an atom. It increases from left to right on the periodic table, decreases from top to bottom in a group. It is higher when the radius is small.

Question 31

Electronegativity

Answer 31

the measure of the ability of an atom to attract shared electrons. It increases from left to right on the periodic table, decreases from top to bottom in a group. It has the same trend as ionization energy. It is low in metals, but high in nonmetals. It is higher when the radius is small.

Question 32

Electron Affinity

Answer 32

the attraction an atom has for shared electrons. This increases from left to right, decreases from top to bottom.

Question 33

Large Negative Ions

Answer 33

indicate that the negative ion formed is very stable

Question 34

Small Negative Ions

Answer 34

indicate that a less stable ion is formed

Question 35

What does a “0” mean in terms of electron affinity?

Answer 35

If you were to add another electron, it would have to go into the next main energy level and would absorb energy to do this, not release it.

Question 36

Ion

Answer 36

charged particles

Question 37

Cation

Answer 37

Positive ions, usually metals. These elements donate valence electrons to another element so that they and the element they are donation to can form a stable compound. The atomic radius is smaller than their parent atom.

Question 38

Anion

Answer 38

Negative ions, usually nonmetals. These elements receive valence electrons from another element so that they and the element donating the electrons can form a stable compound. The atomic radius is larger than the parent atom.