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WorksheetsDeegan & Kim Chem 101 Unit 4
Total questions: 21
Worksheet time: 11mins
Name
Class
Date
1.
How is the f block unique in electron configuration?
a)
There is no difference
b)
The variable at the start of the term is one number fewer than the current period
c)
The variable at the start of the term is two numbers fewer than the current period
d)
Um... what?
2.
Atomic Radius
a)
the total distance from an atom's nucleus to the outermost orbital of electron.
b)
Electrons dance around the nucleus
c)
The nucleus expoldes, and sends out atoms
d)
The total mass of an atom's nucleus that includes the outer most orbital electron.
3.
Define valence electrons?
a)
Valence electrons are the protons in the nucleus of an atom that determine its chemical properties.
b)
The outermost electrons; help determine chemical properties and reactions
c)
Valence electrons are the total number of electrons in all energy levels of an atom.
d)
Valence electrons are the electrons in an atom that are closest to the nucleus and are not involved in bonding.
4.
Define ionization energy?
a)
The energy released when an atom gains an electron.
b)
The amount of energy required to split an atom into two parts.
c)
The amount of energy required to remove an electron from an isolated atom or molecule
d)
The energy needed to move electrons BETWEEN different energy levels within an atom.
5.
What is a period of the period table
a)
Row of Chemical Elements
b)
Column of Chemical Elements
c)
The different elements types
6.
Define Electron Affinity
a)
The amount of energy released when a neutral atom gains an electron
b)
The energy required to remove an electron from an atom.
c)
The tendency of an atom to lose protons when it reacts with other elements.
d)
The energy needed to split an atom into two separate ions.
7.
Define Electronegativity
a)
The measure of how strongly an atom attracts electrons when it is sharing them with another atom in a chemical bond
b)
The ability of an atom to gain protons during a chemical reaction.
c)
The energy required to remove an electron from an atom.
d)
The total number of electrons in an atom's outermost shell.
8.
What is the "Quantum Energy Level?"
a)
The specific amount of energy that an electron in an atom can have. Electrons can "jump" between these specific levels.
b)
The exact position of an electron within an atom at any given time.
c)
The amount of energy required to break an atom into subatomic particles.
d)
The total energy contained in the nucleus of an atom.
9.
What is a group on the periodic table
a)
Column of Chemical Elements
b)
Row of Chemical Elements
c)
Noble Gases
10.
Two Identical Particles cannot occupy the same space at the same time, but due to electron spin two electrons with opposite spin can be in a single orbital.
a)
Pauli Exclusion Principle
b)
Heisenberg Uncertainty Principle
c)
Mendeleev's law
d)
Hund's Rule
e)
The Aufbau Principle
11.
What is a light spectra called when you slow it down with a prism (so you can see the lines)?
a)
Absorption Spectra
b)
Emission Spectra
c)
Continuous Spectra
12.
It is not possible to simultaneously measure an object's momentum and position
a)
Pauli Exclusion Principle
b)
Heisenberg Uncertainty Principle
c)
Mendeleev's law
d)
Hund's Rule
e)
The Aufbau Principle
13.
When writing Orbital Diagrams, what is the rule for drawing the arrows?
a)
All arrows (per term) pointing up must be written before any pointing down
b)
There is no rule
c)
Draw all arrows (per term) pointing down before any point up
d)
Good Luck.
14.
What is the strongest INTRAmolecular Force?
a)
Covalent Bonds
b)
Metallic Bonds
c)
Hydrogen Bonding (VERY RARE)
d)
Ionic Bonds
15.
When Atoms are arranged in increasing atomic number, they show a periodic pattern in their properties
a)
Pauli Exclusion Principle
b)
Heisenberg Uncertainty Principle
c)
Mendeleev's law
d)
Hund's Rule
e)
The Aufbau Principle
16.
Proved Planck's quantum nature of light with his nobel prize winning paper on the photoelectric effect.
a)
Planck
b)
Einstein
c)
Hund
d)
Heisenberg
17.
Each equal energy orbital must have one electron before a second electron with the opposite spin can occupy the same orbital
a)
Pauli Exclusion Principle
b)
Heisenberg Uncertainty Principle
c)
Mendeleev's law
d)
Hund's Rule
e)
The Aufbau Principle
18.
Father of Quantum Mechanics
a)
Planck
b)
Bohr
c)
Einstein
d)
Hund
19.
Added to Pauli's idea of electron spin, by adding that electrons will only pair after the equal energy orbitals are all filled.
a)
Planck
b)
Hund
c)
Heinsenberg
d)
Pauli
20.
His work gives us the idea that no matter how carefully we observe one aspect of an atom, we can never know everything about the current state of the atom.
a)
Planck
b)
Bohr
c)
Heisenberg
d)
Schrodinger
21.
An electron will occupy the lowest energy orbital that is available in the atom
a)
Pauli Exclusion Principle
b)
Heisenberg Uncertainty Principle
c)
Mendeleev's law
d)
Hund's Rule
e)
The Aufbau Principle
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