Indicate whether the following properties increase or decrease from left to right across the periodic table. a. atomic radius (excluding noble gases).
Periodic Trends Worksheet. Directions: Use your notes to answer the following questions. 1. Rank the following elements by increasing atomic radius: carbon, ...
Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum. 3). What is the difference between electron affinity and ionization ...
Exceed to Succeed. Worksheet: Periodic Trends. 1. ATOMIC RADIUS. For each of the following sets of atoms, rank the atoms from smallest to largest atomic radius. a. Li, C, F b. Li, Na, K c. Ge, P, O d. C, N, Al e. Al, Cl, Ga. 2. IONIC RADIUS. For each
For each of the following, circle the correct element. Li. Si. S metal. N. P. As smallest ionization energy. K. Ca. Sc largest atomic mass. S. Cl. Ar member of the halogen family. Al. Si. P greatest electron affinity. Ga. Al. Si largest atomic radius
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Name___________________. Worksheet: Periodic Trends. Period__________________. ____1. Which statement best describes Group 2 elements as they are considered in order from top to bottom of the. Periodic Table? (A) The number of principal energy levels
Periodic Trends Worksheet #4.doc. Periodic Trends Worksheet #4. 1. Describe the atomic size trends seen in the periodic table by both Period and. Group. Explain WHY for each of these trends. 2. Describe the electron affinity trends seen in the period
Atomic Structure and Periodic trends Worksheet (2 points for each question). Complete with a partner and pass in one. First. Ionization Energy. (kJ mol-1). Second. Ionization Energy. (kJ mol-1). Third. Ionization Energy. (kJ mol-1). Element 1. 1,251.
Periodic Trends and Compounds Review Worksheet Answers. Use your text and any other reference that you need except asking someone else to give you the answer. Which group tends to form 1+ ions? alkali metals. Which group tends to form 2+ ions? alkali
Chemistry I 2005
Worksheet 4-3 Periodic Trends
Glencoe Chemistry pp.163-169 ATOMIC RADIUS 1. What trend in atomic radius do you see as you go down a group/family on the periodic table?
2. What causes this trend?
3. What trend in atomic radius do you see as you go across a period/row on the periodic table?
4. What causes this trend?
5. Circle the atom in each pair that has the largest atomic radius. a)
IONIZATION ENERGY 6. Define ionization energy.
7. Is it easier to form a positive ion with an element that has a high ionization energy or an element that has a low ionization energy? 8. Na+ and Mg2+ ions each have ten electrons surrounding their nuclei. Which ion would you expect to have the larger radius? Explain your answer.
9. a. Explain why it is harder to remove an inner shell electron than a valence electron from an atom. b. Explain why sodium forms a 1+ ion (Na+) but magnesium forms a 2+ ion (Mg2+).
10. What trend in ionization energy do you see as you go down a group/family on the periodic table?
Chemistry I 2005
11. What causes this trend?
12. What trend in ionization energy do you see as you go across a period/row on the periodic table?
13. What causes this trend?
14. Circle the atom in each pair that has the greater ionization energy. a)
ELECTRONEGATIVITY 15. Define electronegativity
16. How does the ionic radius of a nonmetal compare with its atomic radius?
17. What trend in electronegativity do you see as you go down a group/family on the periodic table?
18. What causes this trend?
19. What trend in electronegativity do you see as you go across a period/row on the periodic table?
20. What causes this trend?
21. Circle the atom in each pair that has the greater electronegativity. a)