Orbital Diagrams
Electron Configurations
Name That Element
Electron Dot Diagrams
Mixed Review
Periodic Trends
Periodic Trends 2
100
The s block has how many lines and arrows when filled?
1 line, 2 arrows
100
What is the electron configuration of Lithium?
1s2 2s1
100
What element has the following electron configuration:
1s2 2s2 2p4
What is Oxygen
100
This is the name for the outermost electrons.
What is valence electrons
100
What element is found in period 3, group 2?
Magnesium
100
What is ionization energy?
It's the energy required to remove a valence electron.
100
Which element is bigger: Ca or Se?
Ca
200
The p block has how many lines and arrows when filled?
3 lines, 6 arrows
200
What is the electron configuration of Carbon?
1s2 2s2 2p2
200
What element has the following electron configuration:
[Ar] 4s2 3d9
What is Copper
200
What is the correct electron dot diagram for oxygen?
200
What element is found in period 5, group 14?
Tin
200
What is atomic radius?
It is half the distance between two adjacent nuclei of atoms of the same element.
200
What's the difference between a group and a period? What information can we get from them?
Groups are the vertical columns on the periodic table, periods are the horizontal rows.
Groups tell us the number of valence electrons, periods tell us how many energy levels are used to arrange the electrons.
300
The d block has how many lines and arrows when filled?
5 lines, 10 arrows
300
What is the noble gas electron configuration of Arsenic?
[Ar] 4s2 3d10 4p3
300
What element has the following electron configuration:
[Xe] 6s2 5d1 4f14 5d9 6p2
What is Lead
300
What is the correct electron dot diagram for Xenon?
300
What is the name of the last column on the periodic table?
Noble Gases
300
What is electronegativity?
It's a measure of how strongly an atom attracts electrons.
300
Explain why we observe the periodic trends in atomic radius.
It increases from top to bottom within a group because energy levels are added, which increases the distance between the valence electrons and the nucleus.
It decreases across a period, because nuclear charge increases without adding energy levels, so that increases the attraction for electrons which pulls them in and makes the atom smaller.
400
The f block has how many lines and arrows when filled?
7 lines, 14 arrows
400
What is the noble gas electron configuration of Titanium?
[Ar] 4s2 3d2
400
What element ends on the following electron configuration:
4s1
What is Potassium
400
Atom X has electron configuration 2-8-8-1. How many dots would you place around atom's X Lewis Dot Diagram?
What is 1
400
What noble gas will be in the configuration for neptunium?
Radon
400
What is the periodic trend in atomic radius (both in groups and in periods)?
Atomic radius decreases from left to right within a period and increases from top to bottom within a group.
400
Explain why we observe the periodic trends in ionization energy.
It decreases from top to bottom within a group because energy levels are added, which increases the distance between the valence electrons and the nuclear pull. There are also more core electrons to shield the pull from the nucleus, which makes it easier to remove electrons, making ionization energy decrease.
It increases across a period, because nuclear charge increases without adding energy levels, so that increases the attraction for electrons and makes them harder to remove, which increases ionization energy.
500
Explain what's wrong with each of the orbital diagrams below:
A) 
B)
C)
In A, you are not allowed to have two arrows pointing in the same direction on the same line.
In B, you may not pair electrons up until each line has an electron
In C, you may not put electrons in higher energy orbitals until the lower energy one is filled.
500
What is the noble gas electron configuration of Osmium (Os)?
[Xe] 6s24f145d6
500
What element ends on the following electron configuration:
5f7
What is Americium
500
What is the maximum number of dots that you can place around ANY atom?
What is 8
500
How many valence electrons will arsenic have?
5
500
What is the periodic trend in ionization energy (both in groups and in periods)?
Ionization energy increases from left to right within a period and decreases from top to bottom within a group.
500
Explain why we observe the periodic trends in electronegativity.
It decreases from top to bottom within a group because energy levels are added, which increases the distance between the valence electrons and the nucleus. This weakens the attraction for electrons.
It increases across a period, because nuclear charge increases without adding energy levels, so that increases the attraction for electrons.