Potpourri
Name two elements that are classified as metalloids.
Boron
Silicon
Germanium
Arsenic
Antimony
Tellurium
Polonium
Astatine
Which family of elements has a full valence shell and is inert?
Noble gases.
What is emitted when an electron falls from a higher energy level to a lower one?
A photon of light.
What element has the electron configuration 1s22s22p5
Fluorine
Which group has the highest electronegativity: metals, metalloids, or nonmetals?
Nonmetals
What is an orbital in terms of atomic structure?
A region in space with a high probability of finding an electron.
Which group on the periodic table contains highly reactive metals?
Alkali metals
When is light emitted from an atom?
When electrons move down from from excited state to their ground state.
What is the abbreviated electron configuration for Calcium (Ca)?
[Ar] 4s2
Rank the following atoms from largest to smallest atomic radius: C, F, Be.
Be > C > F.
Which element has the electron configuration [Ne] 3s23p3 and what is its group and period?
Phosphorus (P)
Group 15
Period 3
Identify two characteristics of nonmetals.
Brittle
Dull
Poor Conductors
Most are gasses
Why does hydrogen produce the same emission spectrum every time?
Which element has a complete 4th energy level?
Krypton
Compare the trends for ionization energy and atomic radius across a period.
Atomic radius decreases, while ionization energy increases due to stronger nuclear attraction.
What is the difference between the ground state and the excited state of an electron?
The ground state is the lowest energy state of an electron, while the excited state is any higher energy state due to energy absorption.
Where are the metals, nonmetals, and metalloids located?
What are the names of groups 1, 2, 3-12, 17, and 18.
Metals: Left of stair case.
Nonmetals: Right of stair case
Metalloids: Touching staircase (except aluminum)
1: Alkali Metals 2: Alkaline Earth Metals 3: Transition Metals
17: Halogens 18: Noble Gases
What is the relationship between the distance of an electron from the nucleus and its energy?
The farther the electron is from the nucleus, the more energy it has.
Identify the element with the electron configuration [Kr] 5s24d105p5 and explain why this element is highly reactive.
Iodine (I). It is highly reactive because it is one electron short of a full outer energy level, making it eager to gain an electron.
As you move down a group, what happens to atomic radius and why?
It increases because additional energy levels are added.
What happens to ionization energy as you move across a period from left to right? Why?
Ionization energy increases because the radius of the atom is smaller so electrons are held on to tighter.
Why do potassium and sodium have similar properties?
They belong to the same group, sharing similar electron configurations with one valence electron.
Explain how line spectra support the idea of quantized energy levels (how do line spectra explain how we know that electrons can only exist at specific energy levels).
Specific lines of light correspond to specific amounts of energy being released. This tells us that electrons had to make defined jumps to different energy levels to release these specific energies of light.
Which orbitals are valence electrons found in for main group elements?
s and p orbitals
Why is it easier to remove an electron from a metal than a nonmetal?
Metals have larger atomic radii and lower ionization energies.
Electrons are farther from the nucleus so they are not held on to as tightly