1 / 18

Chapter 8 Review “Covalent Bonding”

Chapter 8 Review “Covalent Bonding”. Honors Chemistry. Chapter 8 Review. What is the correct electron configuration arrangement of the four valence electrons of the carbon atom in a methane molecule (CH 4 ): a) 2s 2 2p 2 , or b) 2s 1 2p 3 ?

griffith-myers
Download Presentation

Chapter 8 Review “Covalent Bonding”

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 8 Review“Covalent Bonding” Honors Chemistry

  2. Chapter 8 Review • What is the correct electron configuration arrangement of the four valence electrons of the carbon atom in a methane molecule (CH4): a) 2s22p2, or b) 2s12p3? • Which noble gas has the same electron configuration as the oxygen in a water molecule?

  3. Chapter 8 Review • When placed between oppositely charged metal plates, the region of a water molecule attracted to the negative plate is the ____. • When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) ____.

  4. Chapter 8 Review • The shape of the methane molecule (CH4) is called ____. • How is a pair of molecular orbitals formed? • Which elements can form diatomic molecules joined by a single covalent bond? • What is a typical characteristic of an ionic compound?

  5. Chapter 8 Review • Experimental evidence suggests that the H-C-H bond angles in ethene, C2H4, are ____ degrees. • A bond that is not symmetrical along the axis between two atomic nuclei is a(n) ____ bond. • Once formed, how are coordinate covalent bonds different from other covalent bonds?

  6. Chapter 8 Review • What causes hydrogen bonding? • How many electrons can occupy a single molecular orbital? • According to the VSEPR theory, molecules adjust their shapes to keep ____ as far apart as possible. • Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen: a) carbon, or b) oxygen?

  7. Chapter 8 Review • How do atoms achieve noble-gas electron configurations in single covalent bonds? • What is required in order to melt a network solid (besides high heat)? • Molecular orbital theory is based upon what model of the atom? • Where are the electrons most probably located in a molecular bonding orbital?

  8. Chapter 8 Review • A molecule with a single covalent bond is: a) CO2, or b) Cl2? • A bond formed between a silicon atom and an oxygen atom is likely to be a(n) ____ bond. • Which of the following diatomic molecules is joined (seemingly) by a double covalent bond: a) O2, or b) N2?

  9. Chapter 8 Review • What causes water molecules to have a bent shape, according to the VSEPR theory? • Which of these elements does not exist as a diatomic molecule: a) Ne, or b) F? • Which of the following elements can form diatomic molecules held together by triple covalent bonds: a) fluorine, or b) nitrogen?

  10. Chapter 8 Review • Which of the following covalent bonds is the most polar: a) H-F, or b) H-N? • What is shown by the structural formula of a molecule or a polyatomic ion? • What is thought to cause the disperson forces?

  11. Chapter 8 Review • What are the weakest attractions between molecules called? • Which type of solid has the highest melting point: a) ionic solids, or b) network solids? • Why do atoms share electrons in covalent bonds?

  12. Chapter 8 Review • When H1+ forms a bond with H2O to form the hydronium ion (H3O1+), this bond is called a coordinate covalent bond because ____. • How many valid electron dot formulas – having the same number of electron pairs for a molecule or ion – can be written when a resonance structure occurs?

  13. Chapter 8 Review • What is the shape of a molecule with a triple bond? • Which of the forces of molecular attraction is the weakest: a) hydrogen bonding, or b) dispersion forces? • In which of the following compounds is the octet expanded to include 12 electrons: a) PCl5, or b) SF6?

  14. Chapter 8 Review • Which of the following bonds is least reactive: a) C-C, or b) H-H? • What is the name given to pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules? • Why is hydrogen bonding only possible with hydrogen?

  15. Chapter 8 Review • What causes dipole interactions? • How many electrons does carbon need to gain in order to obtain a noble-gas electron configuration? • How many covalent bonds are in a covalently bonded molecule containing 1 phosphorus atom and 3 chlorine atoms?

  16. Chapter 8 Review • How many electrons does a nitrogen atom need to gain in order to attain a noble-gas electron configuration? • What is the bond angle in a water molecule? • How many unshared pairs of electrons are in a molecule of hydrogen iodide?

  17. Chapter 8 Review • How many electrons are shared in a single covalent bond? • What is the total number of covalent bonds normally associated with a single carbon atom in a compound? • How many valence electrons does an iodine atom have? • How many unshared pairs of electrons does the nitrogen atom in ammonia possess?

  18. Chapter 8 Review • How many electrons are shared in a double covalent bond? End of Chapter 8 Review

More Related