Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

10. Chemical Bonding

Electron Geometry (Simplified)

Introduction to Chemistry

10. Chemical Bonding

Electron Geometry (Simplified)

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Multiple Choice

Determine the number of electron groups for the following cation:AsBr₂⁺.

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Verified step by step guidance

Identify the central atom in the cation AsBr2+. In this case, the central atom is arsenic (As).

Determine the number of valence electrons for the central atom, arsenic (As). Arsenic is in group 15 of the periodic table, so it has 5 valence electrons.

Consider the charge of the cation. The cation has a +1 charge, which means it has lost one electron. Therefore, subtract one electron from the total valence electrons of arsenic, resulting in 4 valence electrons.

Count the number of atoms bonded to the central atom. In AsBr2+, there are two bromine (Br) atoms bonded to arsenic.

Calculate the total number of electron groups around the central atom by adding the number of bonded atoms (2) and the number of lone pairs. Since there are 4 valence electrons and 2 are used for bonding with Br atoms, 2 electrons remain as a lone pair, resulting in 3 electron groups (2 bonded pairs + 1 lone pair).