Periodic Trends Practice

1. Match the following: Coulombic Attraction The attraction between oppositely charged particles like the protons in the nucleus of an atom and its valence electrons. Atomic Radius The total distance from an atom’s nucleus to the outermost orbital of electron. Ionization Energy Energy required to remove an electron from an atom. Electronegativity The measure of attraction an atom has for electrons in a chemical bond. 2. Place the following elements in order of increasing (smallest to largest) atomic radius: B, Ne, Li, N Li, B, N, Ne Ne, N, B, Li 3. Place the following elements in order of increasing (smallest to largest) atomic radius: Mg, Sr, Be, Ca Be, Mg, Ca, Sr Sr, Ca, Mg, Be 4. Why does atomic radius increase down a group? the number of energy levels increases the number of protons increases the number of energy levels decreases the number of protons decreases 5. Why does atomic radius decrease across a period? the number of energy levels increases the number of protons increases the number of energy levels decreases the number of protons decreases 6. Which element on the periodic table has the largest atomic radius? Fr H He Rn 7. Given the representation of a chlorine atom, which circle might represent an atom of fluorine? Circle B (smaller) Circle C (same) Circle D (larger) 8. Place the following elements in order of decreasing (largest to smallest) electronegativity: Cl, Na, Si, Mg. Cl>Si>Mg>Na 9. Why did you pick the order you did for number 8 above? the number of energy levels increases the number of protons increases the number of energy levels decreases the number of protons decreases 10. The following table shows the electronegativity values for the halogens. The electronegativity is decreasing as you go down the halogen family because the number of energy levels of electrons is increasing causing the force of attraction to be lower. 11. Which element on the periodic table has the largest electronegativity? H He F Fr 12. Place the following elements in order of increasing (smallest to largest) ionization energy: B, N, Li, F Li<B<N<F 13. Why did you pick the order you did for number 12 above? the number of energy levels increases the number of protons increases the number of energy levels decreases the number of protons decreases 14. Which element has the lower ionization energy, rubidium or iodine? rubidium iodine 15. Which two trends does the following diagram represent? atomic radius ionization energy electronegativity 16. Which trend does the following diagram represent? atomic radius ionization energy electronegativity 17. If cations (+) are formed by an atom losing its valence electron(s), would you expect the sodium ion (Na⁺¹ ) to be larger or smaller than the sodium (Na) atom? larger smaller 18. If anions (-) are formed by an atom gaining valence electron(s), would you expect the chloride ion (Cl⁻¹ ) to be larger or smaller than the chlorine (Cl) atom? larger smaller 19. Based on their positions in the periodic table, arrange these ions in order of increasing (smallest to largest) radius: Cl⁻¹, K⁺¹, and S⁻² K⁺¹< Cl⁻¹ < S⁻²