Download Chapter 4 Guided Notes Name: 4.1 Defining the Atom 1. Define

Chapter 4 Guided Notes
Name: _________________
4.1 Defining the Atom
1. Define atom 2. ____________________ was among the first to suggest the existence of atoms. He
believed that atoms were ___________________ and ______________________ .
3. Describe the word origins of atom:
4. Read and consider the four tenets of Dalton’s atomic theory (bottom of p102). Write
them in your own words and draw a picture to illustrate each (use Figure 4.2 to guide
you).
Summary
Illustration
1-
2-
3-
4-
5. According to Dalton’s theory, is it possible to convert atoms of one element into atoms
of another element? Explain.
6. Despite their small size, individual atoms are ________________________________
____________________________________________________________________.
7. Describe the range of the radii of most atoms in nanometer (nm).
8. A sample of zinc with a mass of 130.8 g contains 6.02 x 1023 atoms. Calculate the
mass of a single zinc atom.
a. Use dimensional analysis to solve this problem and express your answer in
scientific notation.
b. Find the error in this problem. (Hint: your periodic table may be of help)
9. Do the “Connecting Concepts” activity in the Section Assessment on p103.
4.2 Structure of the Nuclear Atom
10. Define the following:
a. Electron b. Proton c. Neutron d. Nucleus 11. Draw and label a cathode ray tube.
12. What scientist discovered the electron? _____________________
13. What are the three subatomic particles of an atom? ________, ________, ________.
14. Make a chart showing the charges and relative masses of the 3 subatomic particles.
15. True or False The most massive subatomic particle is the electron.
16. True or False The proton is positively charged & the electron is negatively charged.
17. True or False The proton and electron have approximately the same mass.
18. Most scientists in the early 1900’s, including JJ Thomson, thought it likely that
____________________________________________________________
________________________________________________________.
19. JJ Thomson’s model for the atom is called the _____________________ . Draw a
representation of what that might look like (showing the positive and negative
charges).
20. Summarize the experiment shown in Figure 4.7.
21. Which conclusion did Rutherford draw from the gold foil experiment?
22. The Rutherford atomic model is known as _____________________________ .
23. In the nuclear atom ____________________________________________________
____________________________________________________________________.
24. How is Rutherford’s model is different from Thomson’s?
25. True or False
26. True or False
Most of the atom is occupied by the nucleus.
The nucleus is comprised of protons and neutrons.
4.3 Distinguishing Among Atoms
27. What is the key characteristic that makes elements different from each other?
28. Define the following:
a. Atomic number b. Mass number 29. The number of electrons is equal to ________________ in a neutrally charged atom.
30. Complete Practice Problems 15 and 16 here:
15)
16)
31. Write the equation for calculating the number of neutrons:
32. There are two ways that we’ll be writing out element names and their information,
described at the bottom of p 111. In gold-197, what is the ‘197’? _______________
33. Write the two shorthand notations for an atom of aluminum that has a mass number of
27 grams. (Hint: These are exactly like the ones shown for gold, but using a different
element!)
a)
b)
34. Complete Practice Problems 17 and 18 here:
17)
a.
b.
c.
18)
a.
b.
d.
e.
c.
35. What are isotopes?
36. Complete Practice Problem 19 here:
19)
Oxygen – 16
Oxygen – 17
__________
__________
Oxygen – 18
__________
37. Actual mass values for atoms are so small that ______________________________ .
38. The standard isotope used to develop the atomic mass unit is _________________ .
39. According to Table 4.3, how many stable isotopes of hydrogen are there? ____
40. The atomic mass of an element _________________________________________ .
41. Complete Practice Problems 21 and 22 here:
21)
22)
42. True or False
43. True or False
Nitrogen has an average atomic mass of 14.007 amu. Of the two
stable isotopes, Nitrogen-14 and Nitrogen-15, Nitrogen-15 is more
abundant.
The units used to measure the mass of atoms is atomic mass
units or amu’s.
44. To calculate the atomic mass of an element _________________________________
____________________________________________________________________.
45. Complete Practice Problems 23 and 24 here:
23)
24)
46. What does the periodic table allow?
47. Each horizontal row of the periodic table is called a _________________.
48. Each vertical column of the periodic table is called a _________________.
49. Create a concept map using the terms in the “Organizing Information” section of the
study guide on p.121.