1. Monday, May 1st
Entry Task From 1.2 & 1.3 (ISN 73 & 74), explain how atoms, elements, and compounds are related.
Schedule:
Introduction to atoms
Objective: I can identify the parts of an atom.
Homework
Read 5.1
Please have on desk:
Journal open to chapter 5 vocab, pencil, week 30 entry tasks

2. Atom Notes
– the science that studies the properties of substances and how they react with each other.
Chemistry

3. Review Notes
Matter is made of particles called atoms that are too small to see with the eyes.
Matter can not be created or destroyed.
Matter can be an element, a compound, or a mixture.

4. Review Notes Elements are the simplest substances.
Matter can undergo physical and chemical changes.

5. How small are atoms?
There are 2 x 1022 zinc and copper atoms in an ordinary penny! That is 20,000,000,000,000,000,000,000!

6. Types of Atoms in Earth’s Crust
Hydrogen makes up about 90% of the total mass of the universe.
In Earth’s crust,
47% Oxygen
28% Silicon
12% Other elements
8% Aluminum
5% Iron

7. Types of Atoms in Living Things
Living things are mostly oxygen, carbon, hydrogen, and nitrogen, plus more than 20 other elements.
In humans,
61% Oxygen
23% Carbon
10% Hydrogen
3% Nitrogen
3% Other elements

8. Names and Symbols of Elements
Elements get their names in different ways.
Elements can be named from people, places, and Greek words.
Each element has a unique symbol.

9. Elements have unique atoms
Every atom of a specific element, such as silver, is similar to every other atom of the same element.
Every atom of a specific element is different from an atom of a different element.
How? It’s all about the structure of the atom!

10. What is inside an atom?
Nucleus – the dense center of the atom made of protons and neutrons
Nucleus
Protons p
Neutrons p p p p p

11. Let’s be positive!
Protons – positively charged particles in the nucleus: p+
Nucleus
Protons p
Neutrons p p p p p
Protons have a mass of one amu

12. I don’t get a charge out of you
Neutrons - neutral particles in the nucleus: n0
Nucleus
Protons p
Neutrons p p p p p
Neutrons have a mass of one amu

13. What is on the outside?
Electrons – Negatively charged particles that orbit the nucleus in energy levels: e-
Shell
Nucleus
Protons p
Neutrons p p p
Electrons p p

14. Neutral atoms have balance!
In neutral atoms the # of protons equals the # of electrons, but the neutrons can be different
Shell
Nucleus 5
Protons p 4
Neutrons p p p 5
Electrons p p

15. Forces in the Atom, part 1
Gravity: pulls objects toward one another. It depends on the mass of the object and how far apart the objects are
The force of gravity in atoms is very small.

16. Forces in the Atom, part 2
Electromagnetic Force: protons and electrons are attracted to each other because they have opposite charges

17. Forces in the Atom, part 3
Strong Force: protons repel each other because they have the same charge. The strong force overcomes this repulsion to hold the nucleus together.

18. Forces in the Atom, part 4
The Weak Force: is an important force in radioactive atoms.

19. Tuesday, May 2nd
Entry Task Explain where you would find the proton, electron, and neutron in an atom.
Schedule:
Structure of an atom
Objective: I will diagram the electrons, protons, and neutrons of the first 20 elements
Homework
Complete the handout if not finished in class
Please have on your desk:
ISN

20. Building the building blocks
Structure of an Atom
Building the building blocks

21. First Step...
What element are you trying to build?
The atomic number of the element equals the number of protons in the nucleus.
Place the correct number of protons in the nucleus.

22. Second Step...
In order to have a neutral atom, you need to have balanced charges.
That means the number of electrons equals the number of protons.

23. (after that, it gets messy – you’ll learn about that next year!)
How Do I Arrange the Electrons?
For the first 20 elements, use…
1st energy level holds the first 2 electrons
2nd energy level holds the next 8 electrons
3rd energy level holds the next 8 electrons
4th energy level holds the next 2 electrons
(after that, it gets messy – you’ll learn about that next year!)

24. Finally, Add the Neutrons!
Round the atomic mass to the nearest whole number.
Subtract the atomic number from the atomic mass.
The result is the number of neutrons.

25. Your Turn!
Complete the atom drawing handouts using these four easy steps.

26. Wednesday, May 3rd
Entry Task Identify how many protons, electrons, and neutrons are in Nickel.
Schedule:
The Atom
Objective: I will gain a better understanding of atomic theory and the atom
Homework:
No homework

27. Thursday, May 4th
Entry Task How can you determine the number of protons and electrons in a neutral atom?
Schedule:
Ions
Objective: I can describe cations and anions
Homework:
Ion Practice Set
Re-read 5.1
Please have on desk:
“The Atom” handout

28. How are these atoms the same?
How are these atoms different?
What do we call the atom on the right of the screen?

29. Atoms are the same type and have the same number of Protons (Atomic #)
Atoms have different number of electrons, so a different charge.
Atoms with more or fewer electrons than neutral atoms are called IONS.

30. When some types of compounds are formed atoms may gain or lose electrons

31. CATION
An atom that has lost one or more electrons (has an overall positive charge)
Naming Rule:
element ion

32. CATION
Hydrogen and most metals form cations.

33. A Sodium atom losing an electron
11 Protons
8 Neutrons

34. A Sodium atom losing an electron
11 Protons
8 Neutrons

35. A Sodium atom losing an electron
11 Protons
8 Neutrons

36. A Sodium atom losing an electron
11 Protons
8 Neutrons

37. A Sodium atom losing an electron
11 Protons
8 Neutrons
Sodium Ion

38. ANION Naming Rule: root + “ide” ion
An atom that has gained one or more electrons (has an overall negative charge).
Naming Rule:
root + “ide” ion

39. ANION
Non-metals and occasionally hydrogen form anions.

40. A Fluorine atom gaining an electron
9 Protons
8 Neutrons

41. A Fluorine atom gaining an electron
9 Protons
8 Neutrons

42. A Fluorine atom gaining an electron
9 Protons
8 Neutrons

43. A Fluorine atom gaining an electron
9 Protons
8 Neutrons

44. A Fluorine atom gaining an electron
9 Protons
8 Neutrons

45. An atom gaining an electron
Fluoride Ion
9 Protons
8 Neutrons

46. To summarize,
Cations
Atoms with fewer electrons than “neutral atoms” are called positive ions
Negative Charges are not enough to cancel out Positive Charges
Protons are more abundant than electrons

47. Anions
Atoms with more electrons than “neutral atoms” are called negative ions
Negative Charges more than cancel out Positive Charges
Electrons are more abundant than protons

48. Friday, May 5th
Entry Task Why aren’t the masses of the elements whole numbers?
Schedule:
Isotopes
Objective: I can analyze isotopes of elements
Homework:
Complete activity if not finished in class
Re-read 5.1
Please have on desk:
ISN open to Ion Practice Set

49. How are all of these atoms the same?
How are all these atoms different?
What do we call them as a collective group?

50. The atoms are the same element, have the same number of protons (atomic #) and electrons, are all neutral atoms .
The atoms have a different atomic mass because of a different # of neutrons.
Atoms of the same element with different numbers of neutrons are called ISOTOPES

51. Isotopes
An isotope is designated by the name of the element and the total number of protons and neutrons (atomic mass).
The number of protons stays the same, otherwise it would be a different element.

52. H-1 H-2 H-3 2 ways to write isotopes Or you can write it this way:
Mass of Isotope
Atomic Number
Or you can write it this way:
H-1 H-2 H-3