1. Atoms
Mr. Lopez

2. Benchmark SC.8.P.8.7
SC.8.P.8.7 Explore the scientific theory of atoms (also known as atomic theory) by recognizing that atoms are the smallest unit of an element and are composed of sub-atomic particles (electrons surrounding a nucleus containing protons and neutrons)

3. Atoms Structure and charges SC.8.P.8.7
How they relate to matter
Charges
location
Scientific contribution

4. Assessment Question
A British scientist named J. J. Thomson discovered the electron in He suggested that the atom looked like the model below.
A Both models contain a nucleus and an electron cloud.
B. Both models include negative charge and positive charge.
C. Both models show positive charge spread through an area of the atom.
D. Both models show most of the
mass of the atom at the center.

5. 1. Assessment Question
Atoms are a basic building block of certain types of matter. Atoms make up the elements that combine to form compounds to make up much of what we use every day. Which of these substances is NOT made out of atoms?
A. oxygen
B. protons
C. trees
D. carbon dioxide

6. 2. Assessment Question
What is the smallest particle of an element that has all the chemical properties of the element?
A. an atom
B. a molecule
C. an electron
D. the nucleus

7. 3. Assessment Question Which of these particles is the smallest?
A. an atom
B. a nucleus
C. a proton
D. an electron

8. 4. Assessment Question
Which particle’s mass is similar to the mass of a proton?
A. an atom
B. a nucleus
C. a neutron
D. an electron

9. 5. Assessment Question
The element phosphorus reacts with oxygen to produce a bright flame. Which is the smallest particle that will also react with oxygen to produce a bright flame?
A. a phosphorus atom
B. a phosphorus molecule
C. an electron in a phosphorus atom
D. the nucleus of a phosphorus atom

10. 6. Assessment Question
Consider a wooden chair and a balloon. What do these two objects always have in common?
A. Both are made of atoms.
B. Both have the same mass number.
C. Both are made of the same kind of atom.
D. Both are made of the same number of atoms.

11. 7. Assessment Question
A row of 100 million atoms of a single type would be only about 1 centimeter (cm) long. What occupies most of this space?
A. water
B. nuclei
C. electrons
D. empty space

12. 8. Assessment Question
Which group lists the parts of an atom from the most massive to the least massive?
A. proton, nucleus, electron
B. nucleus, electron, proton
C. electron, nucleus, proton
D. nucleus, proton, electron

13. 9. Assessment question
Angelo drinks a large glass of water every morning when he wakes up. Which statement best describes the chemical makeup of the water Angelo drinks?
A. It is made up of a single atom composed of protons, neutrons, and electrons.
B. It is made up of an electron cloud surrounding a dense nucleus.
C. It is made up of many molecules containing atoms joined together by chemical bonds.
D. It is made up of protons and neutrons arranged in a repeating pattern.

14. 10. Assessment Question
Which of these statements describes a fact about an atom’s nucleus?
A. It is negatively charged.
B. It is smaller than an electron.
C. It is the same size in all atoms.
D. It is made of neutrons and protons.

15. 11. Assessment Question
Which of these statements describes a fact about an electron cloud?
A. It is the most massive part of an atom.
B. It is made up of electrons and neutrons.
C. It is where an atom’s electrons are found.
D. It is located in the center of an atom’s nucleus.

16. 12 Assessment Question
Explain how an atom is related to an element.

17. 13. Assessment Question
Write two or three sentences about how our understanding of atoms today is both similar and different from Thomson’s model.

18. 14. Assessment Question
Marcus wants to use two objects to compare the sizes of a proton and an electron. If he uses a basketball for a proton, which object would best represent an electron?
A. a pea
B. a bowling ball
C. a beach ball
D. a soccer ball

19. Mike is drawing a model of an atom
Mike is drawing a model of an atom. He will draw the electron cloud first, and then he will draw the nucleus. Where will he draw the nucleus of the atom?
A. on the outer edge of the electron cloud
B. among the electrons in the electron cloud
C. between the center of the atom and the electron cloud
D. in the center of the atom, surrounded by the electron cloud

20. 15. Assessment Question
The element lithium (Li) has an atomic mass of 3 and a mass number of 7.
Explain how you know that the diagram above represents a lithium atom.

21. 16. Assessment Question
Elements and compounds are both made up of atoms.
Explain how an atom is related to an element.
How do the properties of an atom compare to the properties of the related element?

22. 17. Assessment Question
The element lithium (Li) has an atomic number of 3.
Identify what each label stands for in the atom model.
Explain how you know that the diagram above represents a lithium atom.

23. How does the atomic theory relate to your life?
18. Assessment
How does the atomic theory relate to your life?
Describe the particles that make up an atom.

24. Atomic Mass, Number SC.8.P.8.7 Identify an element by atomic number
Calculate atomic mass
Calculate atomic number
Identify number of valence electrons
Identify the number of P, N, E in an element to determine if it an isotope
Identify number of valence electrons

25. Benchmark SC.912.P.8.4
SC.912.P.8.4: Explore the scientific theory of atoms (also known as atomic theory) by describing the structure of atoms in terms of protons, neutrons, and electrons and differentiate amongst these particles in terms of mass, electrical charges and locations within the atom.

26. Atomic number/Isotope/Atomic mass
C= 0 copying notes /2 with only your table
H=ask 3 before me
A= concept map with details
M=none
P= Looks like students copying down the concept map, looking for text evidence and details
S= Check for success and ticket if you can make the time as a group.

27. Comparing Particles Masses text evidence 279-280
The mass protons and neutrons are about equal.
Electrons are much smaller about 1,840 electrons equals 1 proton or neutron.
Protons and neutrons make up almost all the mass of an atom.
Atoms are measured by atomic mass units called (amu).

28. Atomic number p.279
The number of protons in the nucleus of an element tells us what type of element it is.
The definition of an element is based on it’s atomic number.
For example oxygen has 8 protons in the nucleus so the atomic number is 8.

29. Isotopes p. 280
Atoms with the same number of protons and different number of neutrons are called isotopes.
The mass number would be the total of protons and neutrons in an atom.
If the number of neutrons changes oxygen will become an isotope. For example oxygen is naturally 16 for atomic mass (8p + 8n = 16). But if you add another neutron it will change to Oxygen-17.
Calculate mass number by adding number of protons and number of neutrons.

30. Explain why all three oxygen’s react the same chemically? P.280
The reason the isotopes react the same is because the number of electrons stay the same which gives it the chemical reactivity.
The only thing different in an isotope is the number of neutrons change.

31. 280 Math Tool Box Copy Chart
Atom
8e-
Isotope
Oxygen-16
Oxygen-17
Oxygen-18
Protons 8
Neutrons 9 10 8 8 8

32. 280 Math Tool Box Copy Chart
Element
Mass number P+ n
Fluorine 10
Argon 40 22
Calcium 41 e- 9 20 19 9 18 18 20 21

33. 1. Assessment
Each element is made up of different atoms. The table below compares two elements.
What do the elements in the table have in common?
A. Atoms in each element have 10 nuclei.
B. Atoms in each element have 10 protons.
C. Atoms in each element have 10 neutrons.
D. Atoms in each element have 10 electrons.
Element 1
Element 2
Atomic number 10 9
Mass number 20 19

34. 2. Assessment
An atom’s mass number is 210 and its atomic number is 85. How many neutrons does the atom have?
A. 85
B. 125
C. 210
D. 295

35. 3. Assessment Questions
Shona knows that two atoms have the same number of protons. What else can she assume about the two atoms?
A. They have the same mass number.
B. They have the same electric charge.
C. They have the same number of neutrons.
D. They have the same chemical properties.

36. 4. Assessment Question
An atom of vanadium (V) has 23 protons and 28 neutrons. How many electrons does a neutrally charged atom of vanadium have?
A. 5
B. 23
C. 28
D. 51

37. 5. Assessment Question
An atom of lead has the atomic number 82 and a mass number of How many neutrons does this atom of lead have?
A. 82
B. 125
C. 207
D. 289

38. 6. Assessment Question
What is the mass number of an atom that has 4 protons, 4 electrons, and 5 neutrons?
A. 4
B. 5
C. 9
D. 13

39. 7. Assessment Question
Any atom that has 13 protons is an aluminum atom. Which statement best describes what would happen if a proton were added to an aluminum atom?
A. The atom would lose electrons.
B. The atom would have a negative charge.
C. The atom would no longer be aluminum.
D. The atom would have a smaller atomic number.

40. 8. Assessment Question
The chart below shows the atomic numbers and mass numbers for two elements. Element 2 has a greater atomic number and mass number than element 1.
Element 1 Element 2
Atomic number
Mass number
How many more neutrons does element 2 have than element 1?
A. 5
B. 9
C. 14
D. 39

41. 9. Assessment Question
An atom of the element gallium (Ga) has 31 protons and 39 neutrons. What is the atomic number of gallium?
A. 8
B. 31
C. 39
D. 70

42. 10. Assessment Question
Why is the mass of an atom’s electrons not included in the atom’s mass number?
A. The electrons move so fast that their mass cannot be measure
B. The electrons’ negative charge cancels out their masses.
C. The electrons’ mass is represented in the atomic number.
D. The electrons are much less massive than the rest of the atom.