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Life on the edge, Exams of Chemistry

Rice UniversityChemistry

How many electrons are in the outermost shell? ... changes from 8 to 18 between the element calcium, Ca, and the element gallium, ... of valence electrons.

Typology: Exams

2022/2023

Uploaded on 03/01/2023

wilbur
wilbur 🇺🇸

212 documents

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Life on the Edge CLASS SET!
Part One: Valence Electrons
Complete the table on the handout, filling in the missing atoms. Then answer the questions below.
1. How does the number of electrons change as you move from left to right across a period?
2. What do all the atoms of Group 1A have in common?
3. List three things that all the atoms of the elements in Period 3 have in common.
4. What happens to the electron count and number of shells when you move from neon, Ne, to sodium,
Na?
5. How many shells of electrons will rubidium, Rb, have? How many electrons are in the outermost shell?
Draw a shell model of a rubidium atom. (You do not need to include the individual protons & neutrons,
just the electrons in the correct shells.)
6. Draw a shell model of an atom with two shells and six electrons. What element is this? How many
electrons are in the outermost shell?
7. Draw a shell model of an atom with three shells and two electrons in the outermost shell. How many
total electrons does this atom have? What element is this?
8. Look at the periodic table and the handout, The Shell Model. Explain why the number of electrons in the
third shell suddenly changes from 8 to 18 between the element calcium, Ca, and the element gallium,
Ga.
9. Calculate the following for the elements silicon, Si, germanium, Ge, and cesium, Cs:
a. Total number of electrons b. # of valence electrons c. # of core electrons
Part Two: Electron Shells & Subshells
The periodic table shown below indicates the subshell into which the outermost, or last electron(s), are placed
for each element. For example, if you relate the drawing of the locations of the electrons for calcium, Ca, with
the periodic table, you will find that the last electrons are placed in the 4s subshell.
CLASS SET- Do NOT write on or take. Available online
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Part One: Valence Electrons

Complete the table on the handout, filling in the missing atoms. Then answer the questions below.

  1. How does the number of electrons change as you move from left to right across a period?
  2. What do all the atoms of Group 1A have in common?
  3. List three things that all the atoms of the elements in Period 3 have in common.
  4. What happens to the electron count and number of shells when you move from neon, Ne, to sodium, Na?
  5. How many shells of electrons will rubidium, Rb, have? How many electrons are in the outermost shell? Draw a shell model of a rubidium atom. (You do not need to include the individual protons & neutrons, just the electrons in the correct shells.)
  6. Draw a shell model of an atom with two shells and six electrons. What element is this? How many electrons are in the outermost shell?
  7. Draw a shell model of an atom with three shells and two electrons in the outermost shell. How many total electrons does this atom have? What element is this?
  8. Look at the periodic table and the handout, The Shell Model. Explain why the number of electrons in the third shell suddenly changes from 8 to 18 between the element calcium, Ca, and the element gallium, Ga.
  9. Calculate the following for the elements silicon, Si, germanium, Ge, and cesium, Cs:

a. Total number of electrons b. # of valence electrons c. # of core electrons

Part Two: Electron Shells & Subshells

The periodic table shown below indicates the subshell into which the outermost, or last electron(s), are placed for each element. For example, if you relate the drawing of the locations of the electrons for calcium, Ca, with the periodic table, you will find that the last electrons are placed in the 4s subshell.

  1. Name two elements in which the valence electrons are in an “s” subshell.
  2. How many electrons can be placed into the 2s subshell?
  3. Name two elements in which the valence electrons are in a “p” subshell.
  4. Name two elements in which the last electron(s) are placed in the 3d subshell.
  5. How many electrons can be placed into the 3d subshell?
  6. A total of 18 electrons can be placed in the 3rd^ shell. Explain why.
  7. An electron configuration is a list of all the subshells that have electrons for a given element. Determine which element is associated with each electron configuration in the following table.

Electron Configuration Element

1s 2 2s 1 a)

1s 2 2s 2 2p^3 b)

1s 2 2s 2 2p^6 3s 2 3p^5 c)

1s 2 2s 2 2p^6 3s 2 3p^6 4s 2 3d^6 d)

[Ne]3s 2 3p^6 4s 2 3d^10 4p^2 e)

[Ar]4s 2 3d^10 4p^6 5s 2 4d^10 5p^4 f)

  1. Refer to the following electron configuration answer the questions below:

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5

a. How many total electrons does this element have?

b. What element is this?

c. How many different shells are represented?

d. How many different subshells are represented?

  1. Write out the electron configuration for the following elements:

a. Magnesium, Mg d. Aluminum, Al

b. Nickel, Ni e. Selenium, Se

c. Barium, Ba f. Uranium, U (see if you can do it!)