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Chapter 16 – Review “Covalent Bonding”






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Chapter 16 – Review “Covalent Bonding”. Milbank High School. Chapter 16 - Review. How many electrons are shared in a single covalent bond? How many valence electrons does an atom of any halogen have? How many electrons are shared in a double covalent bond?
Chapter 16 – Review “Covalent Bonding”

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Slide 1

Chapter 16 – Review“Covalent Bonding”

Milbank High School

Slide 2

Chapter 16 - Review

  • How many electrons are shared in a single covalent bond?

  • How many valence electrons does an atom of any halogen have?

  • How many electrons are shared in a double covalent bond?

  • How many electrons does a nitrogen atom need to gain to attain a noble-gas electron configuration?

Slide 3

Chapter 16 - Review

  • How many unshared pairs of electrons does the nitrogen atom in ammonia (NH3) possess?

  • How many electrons does carbon need to gain to obtain a noble-gas electron configuration?

  • What is the total number of covalent bonds normally associated with a single carbon atom in a compound?

Slide 4

Chapter 16 - Review

  • How many unshared pairs of electrons are there in a molecule of hydrogen iodide?

  • How many covalent bonds are there in a covalently bonded molecule containing 1 phosphorus atom and 3 chlorine atoms?

  • What is the name given to the energy required to break a single bond?

Slide 5

Chapter 16 - Review

  • How do atoms achieve noble-gas electron configurations in single covalent bonds?

  • Why do atoms share electrons in covalent bonds?

  • What is shown by the structural formula of a molecule or polyatomic ion?

Slide 6

Chapter 16 - Review

  • What is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules?

  • Which elements can form diatomic molecules joined by a single covalent bond?

  • Which of these elements does not exist as a diatomic molecule: I, Ne, H, F

Slide 7

Chapter 16 - Review

  • What elements can form diatomic molecules held together by triple covalent bonds?

  • What elements can form diatomic molecules held together by double covalent bonds?

  • A covalent bond in which each atom contributes two electrons is a ___.

Slide 8

Chapter 16 - Review

  • A diatomic molecule with a triple covalent bond is _____.

  • A molecule with a single covalent bond is: CO2 or Cl2?

  • Which noble gas has the same electron configuration as the oxygen in a water molecule?

Slide 9

Chapter 16 - Review

  • What diatomic molecule is joined by a double covalent bond?

  • When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) _______.

  • Once formed, how are coordinate covalent bonds different from normally formed covalent bonds?

Slide 10

Chapter 16 - Review

  • What is true concerning the resonant molecule dinitrogen tetraoxide (or any resonant structure for that matter!)?

  • When do exceptions to the octet rule occur?

  • Substances in which all of the electrons are paired are said to be ______.

Slide 11

Chapter 16 - Review

  • How many unpaired electrons are present in each molecule of a para-magnetic substance?

  • Which of the following types of magnetism is the strongest: paramagnetic; diamagnetic; or ferromagnetic?

  • Which of the following fails to follow the octet rule: fluorine or oxygen?

Slide 12

Chapter 16 - Review

  • In which of the following compounds is the octet expanded to include 12 electrons: SO3or SCl6?

  • What is one way in which compounds that do not follow the octet rule can achieve stability?

  • Which of the following pairs of elements can be joined by a covalent bond: Mg and C; or N and C?

Slide 13

Chapter 16 - Review

  • What type of covalent bond is most stable between small atoms: polar or nonpolar?

  • According to VSEPR theory, molecules adjust their shapes to keep what items as far apart as possible?

Slide 14

Chapter 16 - Review

  • What causes water molecules to have a bent shape, according to VSEPR theory?

  • What is the measure of the tetrahedral bond angle?

  • What is the bond angle in a water molecule?

  • What is thought to cause the dispersion forces?

Slide 15

Chapter 16 - Review

  • Which of the forces of molecular attraction is the weakest?

  • What causes hydrogen-bonding?

  • Why is hydrogen-bonding only possible with hydrogen?


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