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Straighterline General Chemistry 1 LAB CHEM101L Lab 6 Molecular Geometry COMPLETE Worksheet with LAB PHOTOS (New Version August 2024) Scored 100%$10.49
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Straighterline Intro to Chemistry CHEM101L Lab 6 Molecular Geometry COMPLETE Worksheet
with LAB PHOTOS (New Version August 2024) Scored 100%
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Lab Report Format Expectations
Utilize college level grammar and professional formatting when completing this worksheet.
Report all equations in a proper mathematical format, with the correct signs and symbols.
Pre-Lab Questions
1. Describe the difference between valence and core electrons.
DUE TO RELIGIOUS REASONS, ITEMS SUCH AS GELATIN I CANNOT USE THEM OR TOUCH, IN
DEFENSE OF MY FAITH I HAVE USED PAPER.
Valence electrons participate in chemical bonding, but core electrons do not. Furthermore, core
electrons are located in the inner shell, whereas valence electrons are found in the outer shell.
Moreover, a valence electron's energy is different from that of a core (nucleus) electron.
2. What is the octet rule and which elements obey the octet rule?
The octet rule, which is present in elements such as carbon, nitrogen, oxygen, and fluorine,
states that an atom must gain or lose electrons in order to match the electronic structure of the
closest noble gas. An atom is considered to have an incomplete octet if it has at most eight
surrounding electrons.
3. How does VSEPR affect the shape of molecules?
It forecasts the behavior of atoms, indicating that the distribution of valence electron groups
must remain consistent as attainable. By positioning both lone pairs and bonded electron pairs
around the core atom in a way that reduces electrostatic repulsion between them, the theory
determines the stability of the molecule.
4. What effect does the presence of lone-pair electrons have on the bond angles in a molecule?
Bond angles decrease when lone-pair electrons are present in a molecule because they repress
bound pairs, contrary to what would be predicted in the absence of lone pairs. The higher
electron concentration in lone pairs causes bonded pairs to move closer together, which is the
cause of this phenomenon. Because of this, molecules that include lone pairs typically have
smaller bond angles than ones that do not.
, Lab 6 Molecular Geometry CHEM101L
5. Should all of the angles in methane (CH4) be equal? Why or why not?
All bond angles are equal because of the tetrahedral molecular shape, with the angles between
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