Matter and its Changes
1. What is matter?
2. What are the states of matter?
3. Define and describe each state of matter in terms of the particle relationships and
kinetic energy.
4. What are the changes of states of matter? What are their terms?
5. How do we model the changes in states using a heating/cooling curve?
6. What are properties of matter?
7. What are physical changes of matter?
8. What are chemical changes of matter?
9. How do you identify if a chemical or physical change has taken place?
10. State whether the following are Physical (P) or chemical (C) changes and explain how
you know and why.
a) Souring of milk _______
g) Burning of coal _______
b) Rusting of iron _______
h) Pulverizing sugar _______
c) Breaking glass _______
i) Boiling water ________
d) Tarnishing of silver _______
j) Melting ice ________
e) Dissolving salt in water ______
k) Melting paraffin _______
f) Magnetizing iron _______
l) Decaying of food _______
11. How would you know if a chemical change has taken place (in other words, what are
the indicators of a chemical change)?
Phase Changes
The states of matter depend on how far apart the molecules are from each other. Describe the
behavior of matter in each of the following states.
1. Solids –
2. Liquids –
3. Gases –
Matter changes and how it changes is dependent on whether energy is added or removed.
Describe what is happening in each of the following situations:
Solid +
Liquid +
Solid +
Heat
Heat
Heat
→
→
→
Liquid →
Gas →
Gas →
Solid +
Liquid +
Solid +
Heat
Heat
Heat
Phase Change Diagram
Label each of the parts of the heating curve. Draw a particle diagram of what each section of
the heating curve would look like. Describe and explain what is happening in each stage.
Indicate the section of the curve where the melting point
and boiling point occur on the graph.
2. What happens to the temperature during melting and
vaporization?
3. What section(s) on the graph does the kinetic energy
increase?
4. Where on the graph is the water only a solid?
5. Where on the graph is the water vaporizing and condensing simultaneously?
1.
The Model of the Atom
Objectives
1. What is the fundamental building block of matter?
2.
Define an atom and element
3.
What is inside an atom?
4.
State the charges on protons, neutrons and electrons
5.
How do charges relate to each other? That is, what affect does each have on the other?
6.
Explain what it means when an atom is electrically neutral
7. Describe the spatial distribution of electrons and the nucleus within an atom? Knowing this spatial
distribution, how would you describe an atom?
8.
Define and find for any atom the:
a) Atomic number
b) Atomic mass / mass number
c) Number of protons
d) Number of neutrons
e) Number of electrons
f) How is this represented by chemist for each atom?
9.
Describe how atoms of the same element are similar
10. What is an ion?
11. What is an isotope?
12. Using information for the various isotopic forms of particular elements, how is the atomic mass actually
determined?
1.
Periodic Table
How is the periodic table arranged? Where are each of the following found?
Period
Alkalai metals
Group/Family
Alkaline earth metals
Metals
Halogens
Nonmetals
Noble gases
Metalloids
Transition metals
Inner transition metals
2.
What are valence electrons?
3.
How are ions determined using the periodic table?
4.
What is meant by oxidation state?
5.
What are the trends in the periodic table for atomic radius, ionization energy, electronegativity and
reactivity?
Atomic Structure and Periodic
Table Practice Problems
1. What is the charge of a proton? An electron?
2. Which pairs of electrical charges attract? Which pairs repel?
3. The atomic number of an atom is the number of its _____
4. Can helium atoms have different numbers of neutrons? Of protons? Of electrons?
5. Describe in your own words the differences between hydrogen and helium.
6. What is an ion?
7. What are the isotopes of an atom?
8. Which element contains 21 protons?
9. Which element contains 11 protons?
10. Which element contains 104 protons?
11. How many protons are in Carbon (C)?
12. How many protons are in Tungsten (W)?
13. How many neutrons are in an atom of Al-27 (Aluminum-27)?
14. Which element contains 35 protons?
15. Which element contains 18 protons?
16. Which element contains 84 protons?
17. How many protons are in Magnesium (Mg)?
18. How many protons are in Gold (Au)?
19.
What do isotopes of an element have in common? How do they differ?
20. C-12 is an isotope of Carbon; what is its atomic number and its atomic mass number?
21.
Write the atomic symbols for nitrogen-14 and nitrogen-15.
22.
Two atoms are found to contain the same number of neutrons. Can we use
this information to determine that they are the same element? Explain.
23.
The average mass of all fluorine (F) atoms is 18.998 u. Do you think most
fluorine atoms have 9 neutrons or 10 neutrons? Explain.
Use the table below find the average atomic mass of lithium (Li).
24.
Isotope
% Abundance
Atomic Mass
7.59%
6.015121 u
Li-7
92.41%
7.016003 u
Li-6
Use the table below to find the average atomic mass of oxygen (O).
25.
Isotope
O-16
O-17
O-18
% Abund.
99.75%
00.04%
00.21%
Atomic Mass
15.994916
16.999132
17.999153
26. Chromium (Cr) has four stable isotopes. Three of these are: Cr-50 with a percent
abundance of 4.35%; Cr-52 with a percent abundance of 83.8%; Cr-53 with a percent
abundance of 9.5%. What is the percent abundance and mass number of the fourth
isotope?
27. Why are the atomic mass number and the atomic mass different?
28. Cu-63 is an isotope of Copper; what is its atomic number and atomic mass number?
29. O-16 is an isotope of Oxygen; how many neutrons, protons and electrons does it have if
it is electrically neutral?
Write the atomic symbols for phosphorus-30 (P-30) and phosphorus-31 (P-31).
30.
31.
Two atoms are found to contain the same number of protons. Can we use this
information to determine that they are the same element? Explain.
32.
Two atoms are found to contain the same number of electrons. Can we use
this information to determine that they are the same element? Explain.
Use the table below to find the average atomic mass of neon, Ne.
33.
Isotope
Neon-20
Neon-21
Neon-22
34.
% Abundance
90.62%
0.26%
9.12%
Atomic Mass
19.992439
20.993845
21.991384
Use the table below to find the average atomic mass of bromine, Br.
Isotope
Br-79
Br-81
% Abundance
50.69%
49.31%
Atomic Mass
78.9183371
80.9168041
35. What element is located in period 3, group 13?
36. What is atomic number of the element in period 6, group 2?
37. Will the element located at period 6, group 3 have a larger or smaller atomic number
than the element in Question 36?
38. What is the group # and period # for oxygen (O)?
39. What is the atomic number of the element in period 5, group 11?
40. What is the atomic number of the element in period 2, group 18?
41. What is the name of the group on the periodic table that krypton belongs to?
42. Two elements are studied. One has atomic number X and one has atomic number X-2 ( X
minus 2). It is known that element X is an alkaline earth metal. What is the name of the
special group that the X-2 element belongs to?
43. What is the name of the group on the periodic table that magnesium belongs to?
44. What is the name of the group on the periodic table that bromine belongs to?
45. A mystery element is in the same period as sulfur. It has a larger atomic number than
sulfur and is nonreactive. What is the mystery element?
46. Two elements are studied. One has atomic number X and one has atomic number X+2. It
is known that element X is a halogen. What is the name of the group that the X+2
element belongs to?
47. Lithium, sodium, and potassium are in the same group of the periodic table. What do
they all have in common?
48. Put the following elements in order of increasing atomic size:
Ca, Rb, K, O, Sn, As
49. Put the following elements in order of decreasing atomic size:
In, Fr, Br, Te, K, F
50. Put the following elements in order of decreasing atomic size:
S, Sb, Cs, Rb, Cl, Pb
51. As you move down a group, valence electrons reside in higher energy levels. How does
atomic radius change? Explain why.
52. Put the following elements in order of increasing atomic size:
Te, Ca, Sr, O, N, Po
53. Put the following elements in order of decreasing atomic size:
He, S, I, Sn, Ba, Pb
54. Put the following elements in order of decreasing atomic size:
C, As, P, Fr, Rb, O
55. You are working with two unknown elements in the lab: X and Y. You know that X has a
lower ionization energy than Y. Which atom has a smaller atomic radius?
56. Put the following elements in order of increasing first ionization energy:
Li, Rb, K, O, Al, As
57. Put the following elements in order of increasing first ionization energy:
Ga, Fr, Br, Si, Na, F
58. Put the following elements in order of increasing first ionization energy:
Se, Sn, Fr, Rb, Cl, Li
59. You are working with two unknown elements in the lab: X and Y. You know that X has a
larger Zeff than Y and are found in the same period. Which element has a higher
ionization energy?
60. Put the following elements in order of increasing first ionization energy:
Ar, Ca, Mg, O, N, At
61. Put the following elements in order of increasing first ionization energy:
Ne, P, F, Sb, Rb, Pb
62. Put the following elements in order of increasing first ionization energy:
He, As, Kr, Fr, S, O
63. You are working with two unknown elements in the lab: X and Y. You know that X has a
lower ionization energy than Y. Which element has the higher electronegativity?
64. Put the following elements in order of increasing electronegativity:
Ca, Rb, K, O, Al, As
65. Put the following elements in order of decreasing electronegativity:
Ga, Fr, Br, Si, Na, F
66. Put the following elements in order of decreasing electronegativity:
Po, Sn, Cs, Rb, Cl, Li
67. You are working with two unknown elements in the lab: X and Y. You know that X has a
higher electronegativity than Y. Which element has a higher Zeff?
68. Put the following elements in order of increasing electronegativity:
Bi, Ca, Mg, O, N, At
69. Put the following elements in order of decreasing electronegativity:
C, K, Br, Sb, Be, Sn
70. Put the following elements in order of decreasing electronegativity:
N, As, Sr, Fr, P, O
Free Response
1. An element has 2 common isotopes. The first isotope has a mass of 68.926 amu
and occurs 60.10% of the time. The second isotope has a mass of 70.925 amu
and occurs 39.90 % of the time. Calculate the atomic mass of this element.
2. Nitrogen has an atomic mass of 14.007 amu. Nitrogen has two common
isotopes. One of the isotopes has a mass of 14.003 amu and a relative
abundance of 99.632%
a) What is the % abundance of the other isotope?
b) What is the mass of the other isotope?
3. Fill in the chart with information on the following atoms.
Element
symbol
Atomic
number
Mass
number
23
51
# of
protons
# of
neutrons
# of
electrons
29
14𝑆𝑖
23
77
115
77
115 3+
49𝐼𝑛
108
47
46
51
61
59
Co
54
24
8
16
8𝑂
80
-1
35𝐵𝑟
4. Hydrogen has two stable isotopes, hydrogen-1 and hydrogen-2 (deuterium)
Isotope
Mass (u)
Natural Abundance
1H
1.007825
?
2H
2.014101
?
a. Which isotope is more naturally abundant? Defend your prediction.
b. Determine the natural abundance of each isotope.