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Chapter 14 – Review Chemical Periodicity. Milbank High School. Chapter 14 - Review. How many electrons are present in the d sublevel of a neutral atom of nickel? (atomic # = 28) What is the electron configuration of sulfur? (atomic # = 16)

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Chapter 14 – Review Chemical Periodicity

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Chapter 14 review chemical periodicity l.jpg

Chapter 14 – ReviewChemical Periodicity

Milbank High School


Chapter 14 review l.jpg

Chapter 14 - Review

  • How many electrons are present in the d sublevel of a neutral atom of nickel? (atomic # = 28)

  • What is the electron configuration of sulfur? (atomic # = 16)

  • What orbital is filled when iodine gains an electron to become a negative ion, I1-?


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Chapter 14 - Review

  • What element has the electron configuration of the following: 1s22s22p63s23p2?

  • What is true of the electron configurations of the noble gases?

  • What is true of the electron configurations of the representative elements?


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Chapter 14 - Review

  • What is another name for the representative elements?

  • What is another name for the transition metals?

  • Each period number in the periodic table corresponds to ________.


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Chapter 14 - Review

  • Representative elements are usually called _______.

  • The category of elements that is characterized by the filling of f orbitals is the ______.

  • Which of the following is a transition metal: cesium or copper?


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Chapter 14 - Review

  • Which of the following groupings contains only representative elements: a) Cu, Co, Cd or b) Al, Mg, Li?

  • How does atomic radius change from left to right across a period in the periodic table?


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Chapter 14 - Review

  • How does atomic radius change down a group in the periodic table?

  • Why is the radius of a positive ion always less than the radius of it’s neutral atom?

  • Why is the radius of a negative ion always greater than the radius of it’s neutral atom?


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Chapter 14 - Review

  • Which group of the periodic table has the highest electronegativity (the tendency to attract electrons to itself, when it is chemically combined with another element)?

  • What factor contributes to the greater atomic size of the higher-atomic-number elements within a particular family?


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Chapter 14 - Review

  • How does the shielding phenomenon affect the relative atomic sizes of elements in the same period?

  • Which of the following elements has the smallest atomic radius: sulfur or chlorine?

  • Atomic size generally ____ as you move left to right in a period.


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Chapter 14 - Review

  • Which of the following has the smallest atomic radius: O or S?

  • The energy required to remove an electron from a gaseous atom is called the _______.

  • What type of electron configurations are particularly stable?


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Chapter 14 - Review

  • For Group 2A metals, which electron is the most difficult to remove from a neutral atom: the first, second, or third?

  • What factor contributes to the lower ionization energy of the higher-atomic-number elements in a family in the periodic table?


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Chapter 14 - Review

  • What factor contributes to the greater ionization energy of the elements on the right side of a period in the periodic table?

  • Which of the following elements has the smallest first ionization energy: potassium or calcium?

  • Which of the following has the lowest electronegativity: Br or Li?


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Chapter 14 - Review

  • Electronegativity generally _____ from left to right across a period.

  • What term is used to describe an atom’s tendency to attract electrons to itself when it is chemically combined with another element?


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Chapter 14 - Review

  • Which of the following elements, when ionically bound to sulfur, attracts electrons less strongly than the sulfur: F or Cs?

  • Compared with the electronegativities of elements at the left end of a period, the elements at the right side of the same period tend to be ___.


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Chapter 14 - Review

  • Which of the following increases with increasing atomic number in Group 2A: atomic radius or number of outermost electrons?


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