University:
University of California, Berkeley
Course:
CHEM 1A | General Chemistry
Academic year:

2024
Views:

233

Pages:

2
Author:

Isabela House

Worksheet: Periodic Trends 1. Which statement best describes group 2 elements as they are considered in order from top to bottom of the Periodic Table?: The number of principle energy levels increases, and the number of valence electrons remains the same. 2. What is the total number of valence electrons in an atom of boron in the ground state?: 3 3. What is the total number of valence electrons in an atom of xenon, Xe?: 8 4. The elements calcium and strontium have similar chemical properties because they both have the same: Number of valence electrons 5. On the Periodic Table of the Elements, all the elements within Group 16 have the same number of: Valence electrons 6. An element with a partially filled d sublevel in the ground state is classified as: A transition metal 7. Which electron configuration represents a transition element?: [Ar]3d54s2 8. Which element in period 5 of the Periodic Table is a transition element?: Ag 9. Which of the following atoms has the largest atomic radius?: K 10. Which noble gas has the highest first ionization energy?: Helium 11. Which sequence of elements is arranged in order of decreasing atomic radii?: Al, Si, P 12. Which list of elements from group 2 on the Periodic Table is arranged in order of increasing atomic radius?: Be, Mg, Ca 13. As each successive element in Group 15 of the Periodic Table is considered in order of increasing atomic number, the atomic radius: Increases 14. The strength of an atom's attraction for the electrons in a chemical bond is the atom's: Electronegativity 15. Which properties are most common in Nonmetals?: High ionization energy and high Electronegativity 16. Which Group 17 element has the least attraction for electrons?: I 17. Which element in Group 16 has the greatest tendency to gain electrons?: O 18. The Group 17 element with the highest electronegativity is: Fluorine 19. As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally: Decreases 20. The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as: First ionization energy 21. Which element is a member of the halogen family?: I 22. Which of the following Group 2 elements has the lowest first ionization energy?: Ba 1/2 23. As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to: Increasing radius and increasing shielding effect 24. Which sequence correctly places the elements in order of increasing ionization energy?: I-Br-Cl-F 25. Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having: A larger nuclear charge 26. Which of the elements has the least attraction for electrons in a chemical bond?: Nitrogen 27. The ability of carbon to attract electrons is: Less than that of nitrogen and oxygen 28. As the elements Li to F in period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the covalent radius of each successive element compare?: The relative electronegativity increases, and the atomic radius decreases. 2/2