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This quiz helps you practice identifying the molecular and electron geometry of chemical compounds using VSEPR theory.
Can you name the geometries that come from the VSEPR Theory for each of these molecules? Test your knowledge on this science quiz and compare your score to others.
Answer the following questions and check your answers below. These problems are for practice only will not be graded. Be sure you know how to draw correct Lewis Dot Structures and are able to correctly predict the electronic arrangement and molecular geometry before going on to the lab assignment.
You can practice writing Lewis structures and determining both the electronic structure (sometimes called the electron-domain geometry) and the molecular structure (sometimes called the shape or the molecular geometry) for molecules.
Electron and Molecular Geometry — Quiz Information. This is an online quiz called Electron and Molecular Geometry. You can use it as Electron and Molecular Geometry practice, completely free to play. There is a printable worksheet available for download here so you can take the quiz with pen and paper.
(i) What is the electron group geometry of the circled/highlighted carbon atom? (ii) What is the molecular geometry of the circled/highlighted carbon atom? (iii) What is the electron group geometry of the circled/highlighted oxygen atom?
Study with Quizlet and memorize flashcards containing terms like Electron groups: 2 Lone Pairs: 0, Electron groups: 3 Lone pairs: 0, Electron groups: 3 Lone pairs: 1 and more.
Identify the major assumption of the VSEPR theory that is used to predict the shape of molecules. Electron pairs repel each other and try to get as far apart from each other as possible. In water, two hydrogen atoms are bonded to one oxygen atom. Why isn't water a linear molecule?
Study with Quizlet and memorize flashcards containing terms like Electron groups: 2 Lone Pairs: 0, Electron groups: 3 Lone pairs: 0, Electron groups: 3 Lone pairs: 1 and more.
Explore molecule shapes by building molecules in 3D! How does molecule shape change with different numbers of bonds and electron pairs? Find out by adding single, double or triple bonds and lone pairs to the central atom. Then, compare the model to real molecules!