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Lewis Dot Structures Critical Analysis Questions:, Lecture notes of Chemistry

Saint Cloud State University (SCSU)Chemistry

Draw the Lewis dot structures for neutral atoms of barium, iodine, and tellurium. 5. Draw the Lewis dot structures for the following ions: sodium (Na1+), ...

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S
Element Symbol
Unpaired valence e-
Paired valence e-
Name ___________________________________________
Date _____________________________ Period ________
Lewis Dot Structures
Critical Analysis Questions:
1. How many valence electrons do the atoms of the elements in Group 3A have? ________________
2. How many valence electrons do the atoms of the elements in Group 6A have? ________________
3. Make a general statement about the number of valence electrons in atoms of elements that are in the same group on the
periodic table.
4. Draw the Lewis dot structures for neutral atoms of barium, iodine, and tellurium.
5. Draw the Lewis dot structures for the following ions: sodium (N a1+), calcium (Ca2+), nitride (N3-), and fluoride (F1-).
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S

Element Symbol

Unpaired valence e-

Paired valence e-

Name ___________________________________________ Date _____________________________ Period ________

Lewis Dot Structures

Critical Analysis Questions:

  1. How many valence electrons do the atoms of the elements in Group 3A have? ________________
  2. How many valence electrons do the atoms of the elements in Group 6A have? ________________
  3. Make a general statement about the number of valence electrons in atoms of elements that are in the same group on the periodic table.
  4. Draw the Lewis dot structures for neutral atoms of barium, iodine, and tellurium.
  5. Draw the Lewis dot structures for the following ions: sodium (Na1+), calcium (Ca2+), nitride (N^3 - ), and fluoride (F^1 - ).

C H H C H

H

H

P Br

Br P Br

Br

The Octet Rule

Octet Rule – When forming compounds atoms gain, lose, or share valence electrons with other atoms so as to acquire the same number of valence electrons as the next noble gas on the periodic table. When sharing valence electrons, all atoms tend to be most stable with a set of 8 valence electrons , with the exception of hydrogen and helium, which are most stable with 2 valence electrons.

4 valence e- 1 valence e- per H (Needs 4 more e-) (Need 1 more e- each) C has 8 valence e- Each H has 2 valence e- Octet Rule Satisfied

5 valence e- 7 valence e- per Br (Needs 3 more e-) (Need 1 more e- each) All atoms have 8 valence e- Octet Rule Satisfied

Critical Analysis Questions:

  1. a) How many valence elecrrons does a sulfur atom have? ____________ b) Draw the Lewis dot structure for S. c) How many unpaired electrons does an atom of sulfur have? ____________ d) How many valence electrons does a sulfur atom need to gain in order to satisfy the octet rule? _____________
  2. a) How many valence electrons does a chlorine atom have? ____________ b) Draw the Lewis dot structure for Cl. c) How many unpaired electrons does chlorine have? ____________ d) How many chlorine atoms can share unpaired electrons with an atom of sulfur in order to form a molecule that satisfies the octet rule for all atoms? ______________
  3. a) Draw the Lewis dot structure for the molecule that would form between one sulfur atom and a minimum number of chlorine atoms.

O H O^ H

H

O H

H

bonding pair lone pair

Line-bond Notation

1 pair of shared electrons = 1 bond = single line

Electron Dot Line-bond Notation Notation

Critical Analysis Questions:

  1. a. Draw the Lewis dot structure for an atom of silicon and an atom of iodine. b. Draw the “Electron Dot Notation” for a molecule of SiI 4. c. Draw the “Line-Bond Notation” for a the molecule of SiI 4. d. How many bonds are in the molecule of SiI 4? ____________ e. How many lone pairs of electrons are in the molecule of SiI 4? _____________
  2. a. Draw the Lewis dot structure for an atom of carbon, hydrogen, and chlorine. b. Draw the “Electron Dot Notation” for a molecule of CH 2 Cl 2. c. Draw the “Line-Bond Notation” for a the molecule of CH 2 Cl 2. d. How many bonds are in the molecule of CH 2 Cl 2? ____________ e. How many lone pairs of electrons are in the molecule of CH 2 Cl 2? _____________