객관식
Draw the best Lewis structure for CH3+. What is the formal charge on the carbon atom?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
객관식
How many lone pairs of electrons are on the As atom in the Lewis dot structure of AsF₃?
A
3 lone pairs
B
1 lone pair
C
0 lone pairs
D
2 lone pairs
검증된 단계별 안내1
Step 1: Begin by identifying the total number of valence electrons available for the molecule AsF₃. Arsenic (As) is in group 15 of the periodic table, which means it has 5 valence electrons. Fluorine (F) is in group 17, so each fluorine atom has 7 valence electrons. Since there are three fluorine atoms, the total number of valence electrons from fluorine is 3 × 7 = 21.
Step 2: Add the valence electrons from arsenic and fluorine to find the total number of valence electrons in AsF₃. This is 5 (from As) + 21 (from 3 F atoms) = 26 valence electrons.
Step 3: Construct the Lewis structure by placing the arsenic atom in the center and arranging the three fluorine atoms around it. Connect each fluorine atom to the arsenic atom with a single bond. Each bond uses 2 electrons, so 3 bonds use 6 electrons.
Step 4: Distribute the remaining electrons to satisfy the octet rule for each atom. Start by completing the octets for the fluorine atoms. Each fluorine atom needs 8 electrons, including the bonding pair. Since each fluorine already has 2 electrons from the bond, place 6 more electrons (3 lone pairs) around each fluorine atom.
Step 5: After placing electrons around the fluorine atoms, check the number of electrons used. You have used 6 electrons for bonds and 18 electrons for the lone pairs on fluorine, totaling 24 electrons. The remaining 2 electrons are placed as a lone pair on the arsenic atom, completing its octet.
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