Chapter 4: The Periodic Table (Patterns)

Metals are commonly on the __________ of the periodic table

Metals are good conductors of ____________

Other properties of Metals: Malleable Ductile Shiny (what’s the other name for shiny?) Lose electrons

Metalloids are on the diagonal line and divide metals and non-metals Metalloids act as good __________

Nonmetals are commonly on the __________ of the periodic table

Ions: have a different number of ___________

Cations have a ________

Anions have a ________

1. Determine the number of electrons in Cr3+

a. 24 electronsb. 27 electronsc. 3 electronsd. 21 electrons

2. Which pair of elements do you expect to be most similar?a. K and Feb. O and Sic. Ne and Nd. Br and I

3. Which element is not a main group element?a. Seb. Moc. Srd. Ba

Isotopes: contain different number of ____________

Two ways to write isotopes:

Atomic Mass equation:

Atomic Mass = + (Fraction of isotope 1 × Mass of isotope 1) + (Fraction of isotope 2 × Mass of isotope 2)+ (Fraction of isotope 3 × Mass of isotope 3)

1. An isotope of an element contains 82 protons and 122 neutrons. What is the symbol for the isotope?

a. 20482Pb

b. 12282Pb

c. 12240Zr

d. 20440Zr

2. Gallium has two naturally occurring isotopes: Ga-69, with mass 68.9256 amu and a natural abundance of 60.11%, and Ga-71, with mass 70.9247 amu and a natural abundance of 39.89%. Calculate the atomic weight of gallium.

3. An element has four naturally occurring isotopes with the masses and natural abundances given here. Find the atomic mass of the element and identify it.

Isotope Mass (amu) Abundance %

1 135.90714 0.192 137.90599 0.253 139.90543 88.434 141.90924 11.13

4. Bromine has two naturally occurring isotopes (Br-79 and Br-81) and has an atomic mass of 79.904amu. The mass of Br-81 is 80.9163amu, and its natural abundance is 49.31%. Calculate the mass and natural abundance of Br-79.

Chapter 5: Naming

Polyatomic Ions:

What is the formula for sodium hydrogen sulfite?a. S(HSO3)2

b. S(HSO4)2

c. NaHSO3

d. NaHSO4

Name the compound SrI2

a. Strontium iodideb. Strontium diiodidec. Strontium (II) iodided. Strontium (II) diiodide

Name the compound NO2

a. Mononitrogen dioxideb. Nitrogen dioxidec. Dinitrogen monoxided. Nitrogen oxide

Name the compound HNO2

a. Hydrogen nitrogen dioxideb. Hydrogen nitratec. Nitric acidd. Nitrous acid

What is the charge of iron in FeCl3?

a. +1b. +2c. +3

Chapter 6: Moles and Mass %

Mole:__________________________________

Avogadro’s number:______________________

1. Convert 3.5 mol of helium to number of helium atoms

2. Convert 1.1 x 1022 silver atoms to moles of silver

3. Determine the number of CH2Cl2 molecules in 25.0g of CH2Cl2a. 0.294 moleculesb. 1.77 x 1023 moleculesc. 1.28 x 1027 moleculesd. 1.51 x 1025 molecules

Molar mass:_____________________________

Mole relationships from a chemical formulaExample: CCl4

4. How many moles of Chlorine are in 3.5mols of CCl4?a. 1 mol Clb. 14 mols of Clc. 3.5 mols of Cld. None of the above

Mass % Composition:______________________

A 0.358-g sample of chromium reacts with oxygen to form 0.523 g of a metal oxide. What is the mass % of chromium inside the metal oxide?

a. 68.5%b. 86.5%c. 63.5%d. 78.5%

What is the mass percentage of K in KBr? Now what about the mass of K in 35.5g of KBr?

Empirical Formula:

Molecular Formula:

Remember: molecular formula is always a whole number multiple of the empirical formula

What is molecular formula for fructose (a sugar found in fruit) from its empirical formula, CH2O, and its molar mass, 180.2 g/mol.

a. C6H12O6

b. C2H8O3

c. CH2Od. C4HO3

A compound is 52.14%C, 13.13%H and 34.73%O by mass. What is the empirical formula of the compound?

a. C2H8O3

b. C2H6Oc. C4HO3

d. C3HO6

Scientists and what they discovered in their experiments: Rutherford: Gold foil: Discovered atoms are mostly empty space J.J. Thomson: Cathode Ray Tube: Discovered the electron Millikan: Oil Drop: Found the mass and charge of an electron Dalton: Dalton’s atomic theory