How are electron arrangements described by Lewis structures, orbital diagrams, and electron configurations? (What do I already know)
Where are the electrons found in a neon atom? Use the drawing tools to show.
Match the following terms or processes with the best definition.
| Stavka koja se može prevući | arrow_right_alt | Odgovarajuća stavka |
|---|---|---|
energy level | arrow_right_alt | subatomic particle with a negative charge |
electron | arrow_right_alt | subatomic particle with a positive charge |
proton | arrow_right_alt | smallest particle of matter that retains its identity in a chemical reaction |
atom | arrow_right_alt | region around a nucleus where electrons are likely to be found |
Classify SOME of the following as characteristics of either carbon or oxygen by dragging them to the correct column.
4 valence electrons
6 valence electrons
8 valence electrons
Contains 6 protons
Contains 12 protons
1s22s22p2
1s22s22p4
Carbon
Oxygen
What Is the Configuration of Electrons Within an Atom? (Type what you already know)
We can think of the electron orbitals as patterns of electron density surrounding an atom’s nucleus. The letters (in order) are ______________ and represent different types of orbitals.
s
f
p
d
Each orbital in an atom can hold up to two electrons. According to the Pauli exclusion principle, no two electrons can have exactly the same quantum number. In other words, no two electrons can be in the same place at the same time. Two electrons can occupy the same orbital, but each electron is assigned a “spin” so that it can be identified individually. In electron configuration notation, the first electron added to an orbital is denoted with the up arrow (↑), and the second has a down arrow (↓). The direction of the arrows reflects the spin of each electron. The spins of the two electrons in an orbital are always opposite one another. Some other basic rules apply to electron configuration notation. First, as the atomic number increases, the number of orbitals required for the electrons increases. Also, all the orbitals of one type (s, p, d, or f) within an energy level (1, 2, 3, etc.) must be completely filled before an electron can occupy the next highest orbital. Finally, Hund’s rule states that all the orbitals of the same energy will be filled with one electron before any of the orbitals take on a second electron. This rule means that electrons in nitrogen, for example, are placed in each of the three p orbitals before any two electrons can share an orbital.
What does the Pauli exclusion principle state?
According to the video 'Magnetic and Spin Quantum Numbers', what are the possible values for 'm'?
Watch video in DiscoveryEducation_Chem_2.3_Exp1
According to the video 'Magnetic and Spin Quantum Numbers', what are the possible values for 's'?
Watch video in DiscoveryEducation_Chem_2.3_Exp1
According to the video 'Pauli Exclusion Principle', two electrons can't be at the same place at the same time in an orbital. Which of the quantum numbers would we have to change if they were to share an orbital?
Label the sub-orbital blocks s, p, d, and f
What kind of notation is this: [Ne]3s1 ?
Use the periodic table to match each element with its correct electron configuration shown. Notice that noble gas configurations are used.
| Stavka koja se može prevući | arrow_right_alt | Odgovarajuća stavka |
|---|---|---|
beryllium | arrow_right_alt | [Ne]3s23p5 |
chlorine | arrow_right_alt | [Ar]4s23d7 |
Molybdenum | arrow_right_alt | [He]2s2 |
cobalt | arrow_right_alt | [Xe]4f145d106s1 |
gold | arrow_right_alt | [Kr]4d55s1 |
The closer an orbital is to the atomic nucleus, the higher its energy.
Electrons fill the orbitals in the following order:
| Stavka koja se može prevući | arrow_right_alt | Odgovarajuća stavka |
|---|---|---|
arsenic | arrow_right_alt | 1s22s22p63s23p64s23d9 |
potassium | arrow_right_alt | 1s22s22p63s2 |
Magnesium | arrow_right_alt | 1s22s22p63s23p64s23d104p3 |
manganese | arrow_right_alt | 1s22s22p63s23p64s1 |
copper | arrow_right_alt | 1s22s22p63s23p64s23d5 |
Each energy level can take a limited number of electrons. Match the maximum electron numbers to the correct energy levels.
2 | 8 | 18 | 32 | |
|---|---|---|---|---|
1st | ||||
2nd | ||||
3rd | ||||
4th | ||||
5th | ||||
6th |
The orbitals of one type (s, p, d, or f) within an energy level (1, 2, 3, etc.) can be partially filled before an electron can occupy the next highest orbital.
What does Hund's rule state?
What does the first quantum number, 'n' represent?
The second quantum number is represented by what letter?
What does the second quantum number represent?
There are 4 orbital shapes represented by letters. What are those letters in order from lowest energy to highest energy?
What letter represents the 3rd quantum number and what does it represent?
What letter signifies the 4th quantum number and what does it represent?