Name___________________________________________________Date______________Hour_____
Chapter 4 and 5 Study Guide (Atomic Structure and the Periodic Table)
1. What did Dalton’s model look like? List the parts of his atomic theory.
His model of an atom was a solid sphere.
Parts of the atomic theory:
•
All matter is made up of individual particles called atoms, which can’t be divided.
•
All elements made of atoms
•
Atoms of same element have same mass, atoms of different elements have different masses
•
Compounds have more than one type of element
•
Atoms of different elements always combine the same way in compound
2. What did JJ Thompson discover? Draw/describe his model.
JJ Thompson discovered the electron. “Plum pudding model” evenly scattered charges.
3. What did Millikan discover and draw/describe his model.
Millikan discovered the exact charge and mass of an electron. His model was of an atom was that there were
negative charges scattered in a positive substance.
4. What did Rutherford discover? Draw/describe his model.
Discovered the dense, positive center of an atom. Model was that protons were in center, electrons
moved on the outside.
5. What did Bohr discover? Draw/describe his model.
Electrons moved in energy levels. Nucleus at center, electrons moving in energy levels on the outside.
6. To find the atomic mass what two subatomic particles do you add together?
Protons + nuetrons
7. Atomic number equals the number of _____protons________ and _____electrons____________.
8. What are the three main parts to the atom? Name them, their charge, location and their mass.
Particle
Charge
Electron
Proton
Neutron
+
0
Location
Outside nucleus
Nucleus
Nucleus
Mass
0 amu
1 amu
1 amu
9. What is unique about any given element? Atomic number (number of protons)
10. What is an isotope?
Atom with different numbers of neutrons but the same number of protons
11. Fill in the chart below.
Element
Number of
Protons
Number of
Neutrons
Number of
Electrons
Atomic
Mass
(amu)
Atomic
Number
K
19
20
19
39
19
Ir
77
115
77
192
77
Cu
29
35
29
64
29
Co
27
28
27
59
27
12. Draw a Bohr model for Oxygen.
8 protons, 8 neutrons, 2 electrons in first energy level, 6 in the second energy level
13. Draw a Bohr model for nitrogen
7 protons, 7 neutrons, 2 electrons in first energy level, 5 in the second energy level
14. Draw a Bohr model for Neon.
10 protons, 10 neutrons, 2 electrons in first energy level, 8 in the second energy level
15. What are valance electrons? Electrons found in the outermost energy shell
16. How many valence electrons are in chlorine? Boron? Chlorine = 7, Boron = 3
17. Here are three isotopes of an element:
12C
13C
14C
a. The element is: _____Carbon_____________
b. The number 6 refers to the _________number of protons________________
c. The numbers 12, 13, and 14 refer to the ______mass number__________________
d. How many protons and neutrons are in the first isotope? ____p = 6, n= 6_____________
e. How many protons and neutrons are in the second isotope? ___p = 6, n = 7______________
f. How many protons and neutrons are in the third isotope? _____p = 6, n = 8____________
18. An element has 8 protons and an atomic mass of 18. What element is this? Is it an isotope, how do
you know? The element is oxygen because the atomic number is 8, it is an isotope because it has
10 neutrons
Chapter 5
1. How did Mendeleev arrange the elements on his periodic table?
Increasing atomic mass
2. How are elements arranged on the Modern day periodic table?
Increasing atomic number
3. How are elements classified?
Metals, non-metals and metalloids
4. What are the properties of a metal?
Malleable, shiny, dense, conductive, solid
5. What are the properties of a non-metal?
Gas, less dense, non-conductive
6. Describe the properties of a metalloid.
Mix of metal and non-metal properties
7. Where do we find metals on the periodic table?
To the left of the metalloids
8. Where do we find non-metals on the periodic table?
To the right of the metalloids
9. Where do we find metalloids on the periodic table?
Along the stair-step line between the metals and the metalloids
10. Describe the reactivity of Group 1A.
Very reactive!
11. Group 1A are called the ______Alkali Metals_____________.
12. Group 2A are called the ______Alkaline Metals_____________.
13. Group 8A are called the________Noble Gases____________.
14. Describe the reactivity of the noble gases.
Very unreactive because of full valence shell
15. A row on the periodic table is called a _______period________________.
16. A column on the periodic table is called a _____group_________________.