CHM 130, Dr. Debbie, HW #1b
Due Wed., Feb 19th
Names: __KEY___________________
Chapters 3, 4, and 5
1. List two defining characteristics (qualities) of the three states of matter
a. Solid: __atoms are tightly packed; atoms vibrate in place but don’t move____
b. Liquid: __organized chaos; have defined volume but take the shape of container___
c. Gas: ___atoms/molecules are widely spaced; atoms/molecules move freely___
2. Identify as element, compound or mixture:
a___element_
b____compound___
c____element
d___mixture______
3. Complete this Table
Element
Symbol
P
Br
Phosphorus
State of matter
at room temp
Solid
Diatomic? Yes
or No?
No
Metal, semimetal or
nonmetal?
Nonmetal
Bromine
Liquid
Yes
nonmetal
Name
4. How many of each type of atom and total atoms are in lactic acid, CH3CH2OHCO2H?
a. C: __3___
b. H: ___7___
c. O: ___3___
d. total: ___13___
5. What is the chemical formula for butane, C4H10, after it boils? __ C4H10 __
6. What are the six physical changes: melting, freezing, boiling, condensation, deposition, sublimation.
7. The Law of Conservation of Mass states that: matter cannot be created or destroyed.
8. The Law of Conservation of Energy states that: energy cannot be created or destroyed.
9. Briefly describe the contribution made by each scientist below
a. Dalton: atomic theory (still mostly true)
b. Thomson: Plum pudding model (discovery of electrons)
c. Rutherford: presence of small, dense, positively charged nucleus in atoms
d. Planck: energy of photons is quantized (can only exist at certain energy values)
e. Bohr: planetary model of electrons around the nucleus in an atom
10. Which subatomic particle in an atom has a -1 charge? __electron_ +1 charge? __proton_
11. The atomic number for an atom is the same as the number of _protons_ in the nucleus.
CHM 130
Spring 2014
Hmwk 1b
12. Complete this table:
Atom
# protons
# neutrons
# electrons
mass number
Copper-64
29
35
29
64
11
12
11
23
23
Na
13. Circle the atoms that are isotopes: carbon-12
boron-12 nitrogen-14
boron-10
14. If a wave has a very long wavelength, then it will have a _low_ frequency. (high or low)
15. If photons in a wave have a high frequency, then they will have a _high_ energy. (high or low)
16. List the letter designations for the 4 sublevels/subshells: ____s, p, d, and f______
17. The third energy level or shell of an atom has how many sublevels or subshells? _3_
18. A d sublevel or subshell contains how many orbitals? __5__
19. How many electrons are in an orbital? __2__
20. Complete the electron configurations for the following atoms.
a. B ___1s22s22p1_ b. K __1s22s22p63s23p64s1___
c. S __1s22s22p63s23p4___
21. Horizontal rows on the periodic table are called _periods_ and vertical columns are called __groups__.
22. What is the name for Group IA in the Periodic table? _alkali metals___
23. What is the name for Group VIIIA in the Periodic table? __noble gases___
24. What element is the alkaline earth metal in the fourth period? __calcium (Ca)__
25. Which one is the smallest atom? Circle one.
F
S
26. Which element is the most metallic? Circle one. Zn
27. Which element has the largest ionization energy?
F
Ca
F
S
K
Cs
Li
Ca
Cs
K
Br
Cs
28. How many valence electrons do the following atoms have? Mg __2_, S __6___, C __4__
29. Which types of elements have smaller ionization energies, metals or nonmetals? __metals_
30. What is the most common charge for the following? Rb __+1__, I_-1__, N __-3_
31. Nonmetals (lose or gain) __gain__ electrons, have a (positive or negative) __negative__ and become
(cations or anions) __anions__.
32. Complete the electron configurations for the following ions. They are just like the atoms, but have lost
or gained electrons.
a. Mg2+ ____1s22s22p6___
b. Be2+ ____1s2____
c. S2 - ___1s22s22p63s23p6_____
33. K+ ion is isoelectronic with which noble gas? __Ar___
34. Se2- ion is isoelectronic with which noble gas? ____Kr_____
35. Isotopes of an atom differ in the number of (p+, e-, or no) __neutrons__; ions differ from atoms in the
number of (p+, e-, or no)) __electrons__.
CHM 130
Spring 2014
Hmwk 1b