WP Unit 2 Practice: The Atom Name 1. Name, and identify them clearly in your answer, one halogen, one noble gas, one alkali metal, one alkali earth metal, one metalloid, one transition metal and finally one inner transition metal. 2. How many protons, neutrons and electrons does the calcium atom have? How many electrons does calcium have if it has a +2 charge? 3. How many protons, neutrons and electrons does the sulfur atom have? How many electrons does sulfur have if it has a - 2 charge? 4. Gold really has only one stable isotope, but many unstable isotopes of low abundance. Look at the periodic table and answer the following question about Gold, Au, a. Fill in the isotope notation below for the most abundant isotope of gold, i.e. give value for A and Z. b. Fill in the table below for the above gold isotope: Protons Neutrons Electrons Electrons in Au 3+ ion
In an atom, each electron has a fixed energy known as its energy level. For example, n=1, n=2, and n=3 are energy levels. Within each energy level, there are sublevels such as s, p, d, and f. Within each sublevel, there are a certain number of orbitals, s has 1, p has 3, d has 5 and f has 7. 1. What is the maximum number of electrons that can be contained in the first, second, third, and fourth energy levels, respectively? 5. What is the maximum number of electrons in each type of sublevel (s, p, d, and f, respectively)? 6. Write the expanded electron configuration (1s 2 2s 2 2p 6, etc.) for the following elements: a. Sodium: b. Calcium: c. Iron: d. Bromine: e. Oxygen: 7. Write the abbreviated electron configuration ([Ne]3s 2 3p6, etc.) for the following elements: a. Manganese: b. Silver: c. Nitrogen: d. Sulfur: e. Argon: 8. What atom has an orbital-filling diagram that ends with the following? a. b.
9. Determine what elements are denoted by the following electronic configuration: a. 1s 2 2s 2 2p 6 3s 2 3p 4 b. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 c. [Kr] 5s 2 4d 10 5p 3 d. [Xe] 6s 2 4f 14 5d 6 e. [Rn] 7s 2 5f 11 10. Determine which of the following electronic configurations are not valid: a. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 10 4p 5 b. 1s 2 2s 2 2p 6 3s 2 3d 5 c. [Ra] 7s 2 5f 8 d. [Kr] 5s 2 4d 10 5p 5 e. [Xe] 11. Below is a representation of the valence electrons of several period 2 elements (1s 2 2s 2 2p n ). A) Identify which is incorrect. B) Show the corrected electronic configuration. C: N: O: F:
In the correct electron-dot symbol, the electrons are distributed across all sides. 12. How many electrons are present in Helium (He) Fluorine (F) Magnesium (Mg) Sulfur (S) Zinc (Zn) 13. How many valence electrons are present in: Helium (He) Fluorine (F) Magnesium (Mg) Sulfur (S) Zinc (Zn) 14. Write the electron-dot symbol for the elements below. Correct Incorrect lithium scandium oxygen aluminum bromine barium argon phosphorus 15. Copper occurs naturally as 63 Cu and 65 Cu. Which isotope is more abundant? 16. Elment Y has two natural isotopes: Y-63 (62.940 amu) and Y-65 (64.928 amu). Calculate the atomic mass of element Y given the abundance of Y-63 is 69.17%.
17. Calculate the atomic mass for chromium given the following data for its natural isotopes: 50Cr 49.946amu 4.35% 52Cr 51.941amu 83.79% 53Cr 52.941amu 9.50% 54Cr 53.939amu 2.36% 18. Which of the following electron configurations belongs to an atom that is most likely to be involved in an ionic bond? Hint: First use the electronic configuration to identify the elements they represent. a. 1s 2 2s 2 2p63s 2 b. 1s 2 2s 2 2p 6 c. 1s 2 2s 2 2p 6 3s 2 3p 3 d. 1s 2 2s 2 2p 6 3s 2 3p 6 19. Which of the following electron configurations belongs to an atom that is most likely to be involved in a covalent bond? Hint: First use the electronic configuration to identify the elements they represent. a. 1s 2 2s 2 2p63s 2 b. 1s 2 2s 2 2p 6 c. 1s 2 2s 2 2p 6 3s23p 3 d. 1s 2 2s 2 2p 6 3s 2 3p 6 20. In order to achieve a noble gas electronic configuration, nonmetals tend to: a. gain electrons b. lose electrons c. form stable free radicals d. a and c 21. Which of the following compounds are ionic circle them. a. CaCl2 b. CO 2 c. H2O d. NaI e. P 2 O 5 22. Indicate how many electrons will each of the following elements gain or lose, in order to achieve a stable full outer shell (since these outer shells are s and p orbital for 8 electrons this is called an octet). What will be the charge on each element once it gains or loses the electrons? a. lithium d. argon g. phosphorus b. oxygen e. scandium h. fluorine c. bromine f. aluminum i. boron