Unit 1 Study Guide Chemistry. Subatomic particle Charge Relative size

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1 VOCABULARY define the following terms: Unit 1 Study Guide Chemistry 1) Atomic mass- 2) Atomic number- 3) Proton- 4) Neutron- 5) Electron- 6) Electron configuration- 7) Isotope 8) Ion 9) Anion 10) Cation - 11) Isoelectronic - 12) Electronegativity - 13) Ionization energy 14) Atomic radius- 15) Valence electrons- 16) Energy level 17) Orbital- 18) Intermolecular forces 19) Intramolecular forces- 40 multi choice Q Hints: - study old quizzes -study practice worksheets & notes -study for understanding, not memorization ATOMIC STRUCTURE A. COMPLETE THE CHART. Subatomic particle Charge Relative size B. A PICTURE OF AN ION (label the nuclear charge, protons, neutrons, and electrons) C. DRAW A PICTURE OF TWO ATOMS THAT ARE ISOTOPES (label the protons, neutrons, and electrons) How are isotopes different? How are isotopes the same?

What are the rules writing electron configuration and orbital diagrams? F.

2 D. What is the relationship between wavelength and amount of energy released? -label the side that is most energetic (highest energy) -label the region that is least energetic (lowest energy) E. What are the rules writing electron configuration and orbital diagrams? F. Write the electron configuration and orbital diagram for the following: i) Phosphorous ii) iii) Calcium Tungsten PERIODIC TABLE TRENDS A. Color or label the following PERIODIC TABLE FAMILIES on the periodic table: -halogens -alkali metals -alkaline earth metals -noble gasses -transition metals -increasing reactivity Which family is the most reactive? Which family is the least reactive?

3 B. Metal v. Nonmetal COLOR OR LABEL THE FOLLOWING -METALS -NONMETALS -METALLOIDS Label which forms anions Label which forms cations COMPLETE THE CHART CONDUCTIVITY LUSTER BRITTLE MALLEABLE PHASE OF MATTER Location on periodic table Example elements METALS METALLOIDS NONMETALS C. Trends LABEL THE FOLLOWING ON THE PERIODIC TABLE -increasing atomic radius -increasing ionization energy -increasing electron affinity -increasing electronegativity -valence electrons -ionic charge

4 BOND TYPE A. How do you know how many valence electrons an element has? B. How do you know what the ionic charge is for any element on the periodic table? C. How is an ionic bond different then a covalent bond? D. How can you distinguish an ionic compound from a covalent compound? E. What are the rules for naming ionic molecules? Naming covalent molecules? F. What are the rules for writing formulas for ionic compounds? Covalent compounds? G. Rank the bond types in order of strongest to weakest: ionic, nonpolar, metallic and polar. H. Explain how intermolecular forces are different then intramolecular forces? Why are both important? I. Rank the 4 bond types in order of highest melting and boiling points to lowest melting and boiling points. Explain why some molecules require more energy to melt/boil then others. PRACTICE QUESTIONS 1. Which subatomic particles are located inside the nucleus? a. protons and neutrons b. protons and electrons c. neutrons and electrons 2. Which subatomic particles are added together to make up the atomic mass. a. Protons and neutrons b. electrons and neutrons c. protons and neutrons 3. What is the atomic mass of Bromine? What is the atomic number of Bromine? a. 11, 5 b. 5, 11 c. 80, 35 d. 35, 80

5 4. A student performs an experiment and records the data in table format. Which of the following is a true statement? Conductivity Reacts with acid Phase of matter malleable Unknown 1 high Yes Solid Yes Unknown 2 none No Gas No Unknown 3 medium no Solid no a. UNKNOWN 1 IS A METAL, UNKNOWN 2 IS A METALLOID b. UNKNOWN 1 IS A METAL, UNKNOWN 2 IS A METAL c. UNKNOWN 2 IS A METAL, UNKNOWN 3 IS A NONMETAL d. UNKNOWN 2 IS A NONMETAL, UNKNOWN 3 IS A METALLOID 5. MATCH THE ELEMENT TO ITS ELECTRON CONFIGURATION a) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 Re b) [Ar] 4s 2 3d 3 V c) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 Sr 6s 2 4f 14 5d 10 6p 4 Po d) [Xe] 6s 2 4f 14 5d 5 6. RANK THE ELEMENTS IN ORDER OF HIGHEST ELECTRONEGATIVITY TO LOWEST Zn, Kr, Ca, Br 7. RANK THE ELEMENTS IN ORDER OF MOST REACTIVE TO LEAST REACTIVE Ca, Mg, Ba 8. RANK THE ELEMENTS IN ORDER OF INCREASING IONIZATION ENERGY Al, In, Ga 9. RANK THE FOLLOWNG ATOMS IN ORDER OF SMALLEST TO LARGEST RADIUS. Cu, Br, Ca 10. RANK THE FOLLOWING COMPOUNDS IN ORDER OF WEAKEST BOND TYPE TO STRONGEST BOND TYPE CH4, CuCl2, Cl2 11. HOW MANY VALENCE ELECTRONS DO THE FOLLOWING ATOMS HAVE? a. Carbon b. Strontium c. Iodine d. Zinc

6 12. WHICH OF THE FOLLOWING ARE ISOELECTRONIC? (circle all that apply) Ar Ca +2 Mg +2 Kr Cl WHICH OF THE FOLLOWING ARE ISOTOPES? a. Ca-40 and Ca-42 b. Ni-64 and Zn-64 c. Ag-107 and Au-197 and Ar FROM THE FOLLOWING PROPERTIES LISTED, IDENTIFY THE ELEMENT a. high luster, 2 valence electrons, period 3 element b. nonmetal, 3 energy levels, -1 ionic charge 15. HOW MANY ELECTRONS ARE AT EACH ENERGY LEVEL FOR THE FOLLOWING ATOMS? A) Calcium (Ca) B) Tin (Sn) 16. Identify as an ionic compound, polar covalent compound, or nonpolar covalent compound. a) CaCl2 c) F2 e) KCl b) SO2 d) H2O 17. Name the following compounds a) NH 4ClO 3 d) Ca 3(PO 4) 2 g) N 2H 4 b) MgBr 2 e) CaCO 3 h) Na 2SiO 3 c) NF 3 f) Fe(NO 3) 3 i) CuCl Write formulas for the following compounds. (balance charges when necessary) a) Ammonium phosphate f) calcium nitrite b) potassium chromate g) manganese (IV) chloride c) Dinitrogen pentoxide h) carbon tetrabromide d) tetraphosphorous decasulfide i) Potassium sulfate e) Silver acetate j) dinitrogen monoxide k) sodium phosphide

VOCABULARY define the following terms:

VOCABULARY define the following terms: Unit 1 Study Guide Honors Chem 1) Electron configuration- 2) Effective nuclear charge 3) Isotope 4) Ion 5) Anion 6) Cation - 7) Isoelectronic - 8) Halogens 9) Electronegativity