Periodic Trends Worksheet



Name Period Date ________________Periodic Trends ATOMIC RADIUS 1. What trend in atomic radius do you see as you go down a group/family on the periodic table?As you go down in the columns, you increase the atomic radius 2. What causes this trend? Energy levels are added as you go down the periodic table, these energy levels are further away from the nucleus, thus increasing the atomic radius.3. What trend in atomic radius do you see as you go across a period/row on the periodic table? The atoms radius decreases4. What causes this trend? As you go across a row, you add protons to the nucleus of the atom, this causes the attractive force between the positively charged nucleus and the negatively charged electrons to increase. The increase in attractive force causes the valance electrons to be pulled closer to the nucleus, thus decreasing the atomic radius.5. Circle the atom in each pair that has the largest atomic radius. a) Al B b) S O c) Br Cl d) Na Al e) O F f) Mg Ca 6. Put the following elements in order from smallest to largest atomic radius and explain why: C, O, Sn, Sr.O, C, Sn, SrOxygen has the most amount of protons on the smallest energy level, Carbon has the same number of energy levels as oxygen, but has less protons. Thus the pull those electrons feel from the nucleus is reduced, increasing the atomic radius. Tin (Sn) has more protons and electrons on more energy levels than Oxygen and carbon, thus increasing the size of the atoms to fit those excess electrons. Strontium (Sr) is simmlar to oxygen, it has less protons than tin, thus decreasing the pull the nucleus has on the valance elctrons and increasing the atomic radius.ELECTRONEGATIVITY 7. Define electronegativity Electronegativity is a measure of the ability of an atom’s nucleus to attract electrons from a different atomwithin a covalent bond8. How does the ionic radius of a nonmetal compare with its atomic radius? Because you add electrons to the ions of a nonmetal, the negative electrons repulse each other, causing the ions to gain a larger atomic radius. 9. What trend in electronegativity do you see as you go down a group/family on the periodic table? It decreases 10. What causes this trend? The valance electrons get further away from the nucleus, thus decreasing the attractive force between those valance electrons and the nucleus. 11. What trend in electronegativity do you see as you go across a period/row on the periodic table? Electronegativity increases.12. What causes this trend? As you increase the number of protons in the nucleus, the attractive forces between the nucleus and the outer electrons increases, this causes the electronegativity to increase.13. Circle the atom in each pair that has the greater electronegativity. a) Ca Ga b) Li O c) Cl S d) Br As e) Ba Sr f) O SGeneral Questions14. Which group tends to form +1 ions? _____________________alkali (Column 1)15. Which group tends to form +2 ions? ____________________Alkaline earth metals (column 2)_16. Which group tends to form -1 ions? _______Halogens (column 17)____________________17. Which group tends not to form ions or react? _________________Noble gasses (column 18)_18. Based on the concept of periodic trends, answer the following questions for these atoms: Li, Be, Mg, Na. Be able to defend your answers. Which element has the lowest electronegativity? _____Na________________________ Which element has the least metallic character? ____Be___________________________ Which element is the largest atom? ______________Na___________________________19. Based on the concept of periodic trends, answer the following questions for these atoms: P, S, Cl, F. Be prepared to defend your answers. Which element has the highest electronegativity? ___F___________________________ Which element has the least metallic character? ____F___________________________ Which element has the largest ion? ______________P___________________________Based on the concept of periodic trends, answer the following questions for these atoms: Au, Zn, S, Si. Be able to defend your answers. Which element has the highest electronegativity? ____S_______________________ Which element has the most metallic character? ______Au________________________ Which element has the largest atom? _______________Au_______________________Complete the following chart:KMgNeNClSiAtomic #19121071714Period432233Group #128574Family name(if any)Alkali Alkaline earth metalsNoble gasn/aHalogenn/a# of valence e-128574# protons19121071714Metal, nonmetal, or metalloid?MetalMetalNonNonNonMetalloidConducts electricity? (yes/no)State at room temperature?Ion Formed?(positive, negative, none, varies)++None--varies_____f________ metal______c_______ chlorine_______b______ transition elements________d_____ group 1 (column 1 )_________e____ noble gases_____a________ group 2 (column 2)alkaline earth metalsmetals with unpredictable propertiesa halogenalkali metalshas a full outer energy level (shell)loses electrons in bondingInstructions Fill in the arrows below with the following terms: increasing electronegativity, increasing metallic character, increasing atomic radius, 85725032004000increasing nonmetallic character, increasing reactivity, decreasing atomic radius204787540005Increasing electronegativity4000020000Increasing electronegativity15128871658938Increasing electronegativity, increasing non-metallic characteristic Increasing electronegativity, increasing non-metallic characteristic 14208121303338Increasing atomic radius, increasing metallic characteristic Increasing atomic radius, increasing metallic characteristic 79082902051686Decreasing atomic radius4000020000Decreasing atomic radius69926202108836Increasing electronegativity4000020000Increasing electronegativity762000433959000-25654011557000584200115570008077200115570007162800115570002127885111125Decreasing atomic radius/4000020000Decreasing atomic radius/2804160361950decreasing electronegativity4000020000decreasing electronegativity64833511811000 ................
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