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Chemical Bonding Study Guide

This study guide provides practice questions on chemical bonding concepts including: - Predicting ions from the periodic table - Identifying the number of valence electrons in atoms - Distinguishing properties of ionic, covalent, and metallic bonds - Classifying bonds as ionic, polar/nonpolar covalent, and identifying molecular shapes - Explaining concepts like VSEPR theory and what causes metals to be malleable - Drawing Lewis structures and identifying intermolecular forces - Classifying unknown substances as ionic, covalent, or metallic based on experimental tests - Ranking and describing different intermolecular forces and how they impact boiling points

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504 views2 pages

Chemical Bonding Study Guide

This study guide provides practice questions on chemical bonding concepts including: - Predicting ions from the periodic table - Identifying the number of valence electrons in atoms - Distinguishing properties of ionic, covalent, and metallic bonds - Classifying bonds as ionic, polar/nonpolar covalent, and identifying molecular shapes - Explaining concepts like VSEPR theory and what causes metals to be malleable - Drawing Lewis structures and identifying intermolecular forces - Classifying unknown substances as ionic, covalent, or metallic based on experimental tests - Ranking and describing different intermolecular forces and how they impact boiling points

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Unit 4a: Chemical Bonding Study Guide

Practice Questions:
● Explain how to use the periodic table to predict ions that will form.

● What ions will the following elements form:


Na: _____ Se: ______ Mg: _____ N: ______ Li: _____ Ba: ______ I: ______

● How many valence electrons will each of the following neutral atoms have?
P: _____ Ca: _____ Rb: _____ As: _____ Br: _____ H: _____ Mg: _____

● List the properties of substances that have covalent, ionic, or metallic bonds.
C I M

● Identify as either a covalent or ionic bond: CaCl₂ CO₂ K₂O P₂O

● Tell whether the bonds in the following compounds are polar covalent, nonpolar covalent, or ionic.
Use your E.N. value chart. You need to memorize the ranges! (Ex: polar covalent [0.5- 1.6] )
MgO SF₆ BCl₃ H₂O K2S CO₂ IF₅

● Label each molecule below with the appropriate molecular shape. You don’t have to draw them!
○ Identify how many bonds are formed in the molecule and if it has any lone pairs.

● State what VSEPR means and how it works.

● Why are metals malleable? Explain what is happening at the particle level!

● Draw the Lewis Dot Structure and write the formula for the ionic compounds made up of:
Mg and N Na and P Sr and Br
○ What type of intermolecular force holds ionic compounds together in a sample?

● Draw the Lewis Dot Structure of each covalent molecule:


NO3 -1 SiCl₄ H₂Se CO₂ NF₃

➢ Use electronegativity values to predict if the bonds are polar or non-polar.


➢ Add arrows to your models to show any unequal sharing of electrons.
➢ What shape would these molecules be?

● Four unknown solids were tested in the lab to determine if they were ionic or covalent substances.
The results of the test are below. Identify each as ionic, covalent, or metallic.
Substance Melting point Dissolves in Conductive (in Conductive as a I, C or M bonds
water water) solid

Low Can’t Tell No No


Unknown A

High Yes Yes No


Unknown B

High No No Yes
Unknown C

Low No No No
Unknown D

● What unknown from the experiment could be MgCl₂? Which could be Zn?

● List the 4 intermolecular forces, and rank them from strongest to weakest.

● When H is bonded to these 3 elements, it is available for hydrogen bonds.

● Explain why dispersion forces are the weakest.

● Explain what the boiling point would be like for a substance that has ionic forces versus one that
has only dipole forces.

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