UNIT 2 Study Guide Chemistry

VOCABULARY define the following terms:

1) Electron configuration – Shorthand for the arrangement of electrons 2) Ion – Atom that has gained (negative charge) or lost (Meow) an electron 3) Anion – Negatively charged ion b/c gained electron(s) 4) Cation – Meow – Positively charges ion b/c lost electron(s) 5) Electronegativity - Property of atoms describes how “fairly” atoms share electrons 6) Ionization energy – Amount of energy it takes to completely remove an electron from an atom 7) Atomic radius – Size of the atom – Found by dividing distance between nuclei of adjacent atoms. 8) Valence electrons – Electrons in outer most energy level / Responsible for bonding and properties 9) Ionic bond – Bond formed by transfer of electrons 10) Covalent bond – Bond formed by sharing of electrons 11) Periodic table group – Up and down Columns 12) Periodic table family – Up and down Columns

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? Most – Alkali Metals Least – Noble gases

B. Trends

LABEL THE FOLLOWING ON THE PERIODIC TABLE

-increasing atomic radius -increasing ionization energy -increasing electronegativity

C. Metal v. Nonmetal

COLOR OR LABEL THE FOLLOWING

-METALS -NONMETALS -METALLOIDS Label valence electrons – Use Column #

Label IONIC CHARGE Label which forms anions

Label which forms cations

COMPLETE THE CHART by placing a X in the appropriate box

METALS METALLOIDS NONMETALS CONDUCTIVITY Y Depends N LUSTER Y Depends N BRITTLE N Depends Y MALLEABLE Y Depends N PHASE OF MATTER Solid Solid Gas Location on periodic table Left Middle Right Example elements Li & Ca Si & Ge N & O

BOND TYPE

A. How do you know how many valence electrons an element has? Column Number

B. How do you know what the ionic charge is for any element on the periodic table? Think Octets

C. How is an ionic bond different then a covalent bond? Ionic Trade vs Covalent share

D. How can you distinguish an ionic compound from a covalent compound? Metal vs Nonmetal at beginning 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. Ionic – Metallic – Covalent/Polar – Covalent/Nonpolar

PRACTICE QUESTIONS

1. Label the ionic charge for the following elements? a. Cu+2 or +1 b. K+1 c. S-2 d. Kr – None: Noble Gas

2. RANK THE ELEMENTS IN ORDER OF HIGHEST ELECTRONEGATIVITY TO LOWEST

Zn, Kr, Ca, Br Kr – Br – Zn – Ca 3. RANK THE ELEMENTS IN ORDER OF MOST REACTIVE TO LEAST REACTIVE Ca, Mg, Ba Ba – Ca – Mg

4. RANK THE ELEMENTS IN ORDER OF INCREASING IONIZATION ENERGY Al, In, Ga Al – Ga – In

5. RANK THE FOLLOWNG ATOMS IN ORDER OF SMALLEST TO LARGEST RADIUS.

Cu, Br, Ca Ca – Cu – Br

6. RANK THE FOLLOWING COMPOUNDS IN ORDER OF WEAKEST BOND TYPE TO STRONGEST BOND TYPE – Ionic – Polar Covalent – NP Covalent

CH4 , CuCl2 , Cl2 CuCl2 – CH4 – Cl2

7. HOW MANY VALENCE ELECTRONS DO THE FOLLOWING ATOMS HAVE? a. Carbon b. Strontium c. Iodine d. Zinc 4 2 7 2

8. HOW MANY ELECTRONS ARE AT EACH ENERGY LEVEL FOR THE FOLLOWING ATOMS? A) Calcium (Ca) B) Tin (Sn) 1st – 2 1st – 2 2nd – 8 2nd – 8 3rd – 8 3rd – 18 4th – 2 4th – 18 5th - 4 9. FROM THE FOLLOWING PROPERTIES LISTED, IDENTIFY THE ELEMENT a. high luster, 2 valence electrons, period 3 element Mg b. nonmetal, 3 energy levels, -1 ionic charge Cl

10. Identify as an ionic compound, polar covalent compound, or nonpolar covalent compound.

a) CaCl2 _____I______c) F2 _____NPC______e) KCl ____I______

b) SO2 _____PC______d) H2O _____PC______

For the next 6 questions, use the periodic table below.

I II III

IV V

11. Which unknown element would have the highest ionization energy? a. I b. II c. III d. IV e. V

12. Which unknown would have the lowest ionization energy? a. I b. II c. III d. IV e. V

13. Which unknown element would have the highest electronegativity? a. I b. II c. III d. IV e. V

14. Which unknown element would have the smallest atomic radius? a. I b. II c. III d. IV e. V

15. Which unknown element would most likely form an anion? (circle all that apply) a. I b. II c. III d. IV e. V

16. Which of the following unknowns would have a + 1 charge? a. I and II b. II and III c. I and IV d. III and V

17. Name the following compounds

a. NH4ClO3 ammonium chlorate f. Fe(NO3)3 iron (III) nitrate

b. MgBr2 magnesium bromide g. N2H4 dinitrogen tetrahydride

c. NF3 nitrogen trifluoride h. Na2SiO3 sodium silicide

d. Ca3(PO4)2 calcium phosphate i. CuCl2 copper (II) chloride

e. CaCO3 calcium carbonate

18. Write formulas for the following compounds. (balance charges when necessary)

a) Ammonium phosphate (NH4)3PO4 f) calcium nitrite Ca(NO2)2

b) potassium chromate K2CrO4 g) manganese (IV) chloride MnCl4

c) Dinitrogen pentoxide N2O5 h) carbon tetrabromide CBr4

d) tetraphosphorous decasulfide P4O10 i) Potassium sulfate K2SO4

e) Silver acetate AgC2H3O2 j) dinitrogen monoxide N2O

k) sodium phosphide Na3P