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What is electron affinity (Eea), and what's its periodic trend?
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Rank these elements according to first ionization energy from highest to lowest. F, O, C, Be, Li, Ne
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CHEM 131
Chapter 4
| Question | Answer |
|---|---|
| What is electron affinity (Eea), and what's its periodic trend? | It is the energy generally released when an electron is added to an atom. F has a high Eea. |
| Rank these elements according to first ionization energy from highest to lowest. F, O, C, Be, Li, Ne | Ne, F, O, C, Be, Li |
| Rank these elements according to first ionization energy from highest to lowest. As, P, Sb, N | N, P, As, Sb |
| Order Cl, Cs, Na, and Si in terms of increasing electron affinity (absolute values). | Cs, Na, Si, Cl |
| Determine the number of valence electrons for each of the following atoms. C, P, O, Ar | 4, 5, 6, 8 |
| Answer the questions about the characteristics of the elements in Group 1 (the alkali metals). 1. How does this group react with Br? 2. How do these react with water? 3. How do they react with O? 4. Which reacts most vigorously? Li, Na, K, Rb, Cs | 1. A salt is formed (MBr) 2. Violently/rapidly to release hydrogen gas 3. Rapidly to form an oxide 4. Cs |
| Answer the questions about the characteristics of the elements in Group 2 (the alkaline earths). 1. How do they react with Iodine? 2. How do they react with water? 3. How do they react with oxygen? 4. Which reacts most vigorously? Be, Mg, Ca, Sr, Ba | 1. A salt is formed (MI) 2. violently/rapidly (less violent than grp 1A) to release hydrogen gas 3. An oxide is formed (2MO) 4. Ba |
| What is the chemical formula for the compound formed between barium and iodine? | BaI2 (subscript 2) |
| What is the chemical formula for the compound between barium and oxygen? | BaO |
| Identify the generic outer electron configuration for the halogens. | ns2np5 |
| What element forms an ion with an electronic configuration of [Kr] and a –2 charge? | Se |
| Predict the ground-state electron configuration of the following ions. Write your answers in abbreviated form, that is, beginning with a noble gas in brackets. Ru2+ (superscript 2+) W3+ (superscript 3+) | Ru: [Kr]4d6 (superscript 6) W: [Xe]4f14 5d3 (4f superscript 14, 5d superscript 3) |
| How many unpaired electrons are there in Er3+ ? | 3 |
| Rank these atoms and ions according to radius from smallest to largest. Rb- Rb+ Rb | Rb+, Rb, Rb- |
| Which of the following ions are isoelectronic with Xe? I-, Rb+, Te2+, Ba2+ | I-, Ba2+ |
| Which of these are ionic compounds? BrCl NH3 LiBr CaO SO2 Nh4Cl | NH4Cl, LiBr, CaO |
| Rank these ions according to ionic radius. As3-, Se2-, As3-, Sr2+, Rb+ | Sr2+, Rb+, Br-, Se2-, As3- |
| Which of the following would be expected to have the smallest lattice energy? SrI2, Na2S, KBr, MgCl2, InSb, AlCl3, RbI | RbI |
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eacrick