Orbital Diagrams
Electron Configurations
Name That Element
Vocab
Mixed Review
Periodic Trends
Periodic Trends 2
100
The s block has this many orbitals and arrows when filled
What is 1 orbital, 2 arrows?
100
What is the electron configuration of Lithium?
1s2 2s1
100
This element has the following electron configuration:
1s2 2s2 2p4
What is Oxygen (O)?
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 this many lines and arrows when filled
3 orbitals, 6 arrows
200
What is the electron configuration of Carbon?
1s2 2s2 2p2
200
This element symbol has the following electron configuration:
[Ar] 4s2 3d9
What is Copper (Cu?)
200
This is the name of a negative ion
What is an anion?
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?
Groups are the vertical columns on the periodic table, periods are the horizontal rows.
300
The d block has how many orbitals and arrows when filled
What is 5 lines, 10 arrows?
300
What is the noble gas electron configuration of Arsenic?
[Ar] 4s2 3d10 4p3
300
This element has the following electron configuration:
[Xe] 6s2 5d1 4f14 5d9 6p2
What is Lead (Pb)?
300
The element in group 4 period 3 belongs to this family
What is there is no element there?
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
Explain what's wrong the orbital diagram: 
You are not allowed to have two arrows pointing in the same direction on the same line.
400
Predict the charge that this element would form when it loses electrons: [Ar] 4s² 3d¹⁰ 4p⁶ 5s2
What is +2?
400
This element ends on the following electron configuration:
4s1
What is Potassium (K)?
400
This is the energy either lost or gained when acquiring an electron.
What is electron affinity?
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
Draw the orbital diagram for Cl-1
I will check
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
This is the name of the configuration that all atoms wish to achieve, normally through ionization.
What is an octet?
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.