Chapter 14 – Review Chemical Periodicity

1. Chapter 14 – ReviewChemical Periodicity Milbank High School

2. 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-?

3. 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?

4. 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 ________.

5. 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?

6. 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?

7. 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?

8. 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?

9. 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.

10. 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?

11. 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?

12. 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?

13. 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?

14. 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 ___.

15. Chapter 14 - Review • Which of the following increases with increasing atomic number in Group 2A: atomic radius or number of outermost electrons?