Name:______

Date:______Per. #:______

Chemistry – Unit 2

HW 2.2 – The Periodic Table Read pg. 11-17, 133-136

Directions: Identify the correct substance, particle, mixture, and state. See below for examples.

Possible Responses

Type of Substance
Element, compound, or mixture? / Type of Particle(s)
Atoms, molecules, ions, or formula units? / Type of Mixture
Homogeneous, heterogeneous, or N/A? / State(s) of Matter
Solid, liquid, gas?
Volume & Shape
definite/indefinite?

Example

Sample: A glass of salt water.
Particles: H2O, Na+, Cl-
Type of Substance
mixture / Type of Particle(s)
Molecules, ions / Type of Mixture
homogeneous / State(s) of Matter
liquid
Volume: definite
Shape: indefinite

1)

Sample: some crystals of copper chloride
Particles: CuCl2
Type of Substance / Type of Particle(s) / Type of Mixture / State(s) of Matter
Volume:
Shape:

2)

Sample: a flask filled with fluorine gas
Particles: F2
Type of Substance / Type of Particle(s) / Type of Mixture / State(s) of Matter
Volume:
Shape:

3)

Sample: stainless steel alloy
Particles: Fe, Cr
Type of Substance / Type of Particle(s) / Type of Mixture / State(s) of Matter
Volume:
Shape:

4)

Sample: A solution of sodium hydroxide
Particles: H2O, Na+, OH-
Type of Substance / Type of Particle(s) / Type of Mixture / State(s) of Matter
Volume:
Shape:

5)

Sample: some sand mixed with some sugar
Particles: SiO2, C12H22O11
Type of Substance / Type of Particle(s) / Type of Mixture / State(s) of Matter
Volume:
Shape:

6)

Sample: A diamond
Particles: C
Type of Substance / Type of Particle(s) / Type of Mixture / State(s) of Matter
Volume:
Shape:

7)

Sample: gasoline and water (hint: they don’t dissolve together)
Particles: H2O, C8H10
Type of Substance / Type of Particle(s) / Type of Mixture / State(s) of Matter
Volume:
Shape:

8)

Sample: carbon dioxide
Particles: CO2
Type of Substance / Type of Particle(s) / Type of Mixture / State(s) of Matter
Volume:
Shape:

Numbers 9-12 are questions about the reading. You may be tested on this information.

9.a) Who is credited with developing the method that led to the determination of standard relative mass?

b) Who discovered periodic law?

c) Who established atomic numbers as the basis for organizing the periodic table?

10. State the periodic law.

11. Name three sets of elements that have been added to the periodic table after Mendeleev’s time.

12. How do the atomic numbers of the elements within each of Groups 1, 2, and 13-18 of the periodic table vary? (refer to figure 4 as a guide)

13. Complete the following table:

Symbol / Name / Block / Atomic # / Group # / Group Name
Na
Ar
Au
Ba
Si
Cl
U

14. The notation used is shown below.

Directions: Remember that the number of neutrons is found by subtracting the atomic number from the atomic mass. Using this principle, find the number of protons, neutrons, and electrons in each isotope. Assume each atom has an overall neutral charge.

Example:

/ 6 protons / 6 neutrons / 6 electrons
Isotope / # protons / # neutrons / # electrons