Ch 3 Matter and Atomic Structure Lesson 1

Atoms

Name: ______Date: ______Period: ______

Focus Question: ______

Notes:Your teacher will give you notes on atoms. Skip to the Directed Reading.

Directed Reading: Read pp. 53-57. Answer the following questions.

  1. What is an element? ______
  1. How many elements occur naturally on Earth and in the stars? ______
  1. What is an atom? ______
  1. Where is the nucleus of an atom? ______
  1. The Parts of an Atom: Fill in the Chart …

Subatomic Particle / Where in the atom is it? / What type of charge does it have? / Does it have mass?
1. Proton
2. Neutron
3. Electron
  1. Define: atomic number. ______
  1. Define: atomic mass. ______
  1. FITB: Atomic number = the number of ______= the number of electrons
  1. What are valence electrons? ______
  1. A Hydrogen Atom: Look at Figure 3-1 on page 56. Draw and label Part A and copy its caption below.

Picture of Hydrogen / Caption
  1. An Oxygen Atom: Look at Figure 3-1 on page 56. Draw and label Part B and copy its caption below.

Picture of Oxygen / Caption
  1. An Aluminum Atom: Look at Figure 3-1 on page 56. Draw and label Part C and copy its caption below.

Picture of Aluminum / Caption

Practice: For each element … Fill in the information and draw it.

  1. Helium
  2. Atomic number - ______
  3. Number of protons - ______
  4. Number of electrons - _____
  5. Atomic mass - ______
  6. Number of neutrons – ______( ______- ______)

Atomic mass minus atomic number

  1. Lithium
  2. Atomic number - ______
  3. Number of protons - ______
  4. Number of electrons - _____
  5. Atomic mass - ______
  6. Number of neutrons – ______( ______- ______)

Atomic mass minus atomic number

  1. Nitrogen
  2. Atomic number - ______
  3. Number of protons - ______
  4. Number of electrons - _____
  5. Atomic mass - ______
  6. Number of neutrons – _____ ( ______- ______)

Atomic mass minus atomic number

Ch 3 Matter and Atomic Structure Lesson 2

Elements and the Periodic Table

Name: ______Date: ______Period: _____

Focus Question: ______

Notes:

Directed Reading:Read pp. 58-59. Answer the following questions.

  1. What is an isotope? ______
  2. Give an example of isotopes. ______
  3. What is atomic mass? ______
  4. What is radioactivity? ______
  5. Draw and label Figure 3-3. Write the caption.

The Periodic Table

Draw Figure 3-4. You do not need to write the caption.

Abundance of Elements

Review:

  1. What are the two most common elements of the universe? (List percentages.) ______
  1. What are the two most common elements of the Earth’s crust? (List percentages.) ______
  1. List the other 6 elements that are prevalent in Earth’s crust.
  2. ______
  3. ______
  4. ______
  5. ______
  6. ______
  7. ______
  1. Look at p. 917. Pick three elements that prevalent in Earth’s crust and draw their information inside the “boxes” below.

Ch 3 Matter and Atomic Structure Lesson 3

Covalent Bonds

Name: ______Date: ______Period: ______

Focus Question: ______

Notes:

Directed Reading: Read pages 60-62. Answer the following questions.

  1. What is a compound? ______
  1. What is a chemical bond? ______
  1. What is a covalent bond? ______
  1. What is a molecule? ______
  1. FITB: Polar Bonds p. 62 - When atoms in a covalent bond do not share electrons equally, they form ______bonds. A polar bond has a ______and a ______end.
  1. The Formation of a Water Molecule. Draw Figure 3-6 below (NEATLY, please!). Label the two hydrogen atoms, the oxygen atom, and the water molecule.

The Formation of a Water Molecule

  1. A Polar Molecule. Draw and label Figure 3-7 below. Write the caption in the box next to your picture.

A Polar Molecule

/

Caption

Practice: Show the covalent bonding of one hydrogen atom to another hydrogen atom to make a hydrogen molecule (which is how hydrogen gas exists in nature). Remember: Hydrogen has an atomic number of 1. Draw protons and electrons only.

Ch 3 Matter and Atomic Structure Lesson 4

Ionic Bonds

Name: ______Date: ______Period: ______

Focus Question: ______

Notes:

Directed Reading: Read pages 62-63. Answer the following questions.

  1. What is an ion? ______
  1. FITB: Ions- p. 62.
  1. An atom in which the outermost energy level is less than half-full tends to ______its valence electrons to become a ______ion. An example of this is a sodium ion. Write the symbol for a sodium ion: ______. Then draw it in the box below.

Positive Sodium Ion

  1. An atom in which the outermost energy level is more than half-full tends to fill its outermost energy level by ______one or more needed electrons to become a ______ion. An example of this is a chlorine ion. Write the symbol for a chlorine ion: ______. Then draw it in the box below.

Negative Chlorine Ion

  1. An atom in which the outermost energy level is exactly half full may form either a ______or ______ion. An example of this is a silicate ion. Write the symbol for a silicate ion: ______
  1. What is an ionic bond? ______

Practice: Draw the NaCl only of Figure 3-8.

NaCl

Ch 3 Matter and Atomic Structure Lesson 5

Metallic Bonds

Name: ______Date: ______Period: ______

Focus Question: ______

Notes:

Directed Reading: Read pages 64. Fill in the Blanks …

  1. Most compounds on Earth are held together by ______or ______bonds.
  1. In METALS, the ______electrons are shared by all the atoms.
  1. You could think of a METAL as a group of positive ______floating in a sea of ______electrons.
  1. The positive ions of the METAL are held together by the ______between them.
  1. A METALLIC bond allows METALS to conduct ______because the ______can move freely throughout the entire solid metal.

Ch 3 Matter and Atomic Structure Lesson 6

Chemical Reactions

Name: ______Date: ______Period: ______

Focus Question: ______

Notes:

Directed Reading: Read page 64.

  1. Remember that atoms gain, lose, or share electrons to become more ______.
  1. What is a chemical reaction? ______
  1. FITB: Chemical reactions are described by chemical ______.
  1. FITB: You must balance an equation by showing an ______number of atoms for each element on each side of an equation. This is because the same amount of matter is present both before and ______the reaction.

Practice: Practice writing the following equations. Be sure to balance them!

  1. Iron (Fe) combines with oxygen (O2) to yield rust (FE2O2).
  1. Hydrogen (H2) combines with oxygen (O2) to yield water (H2O).
  1. Carbon (C ) combines with oxygen (O2) to yield carbon dioxide (CO2).

Ch 3 Matter and Atomic Structure Lesson 7

Mixtures and Solutions

Name: ______Date: ______Period: ______

Focus Question: ______

Notes:

Directed Reading: Read page 65.

  1. What is a mixture? ______
  1. FITB: When a mixture’s components are easily recognizable, it is called a ______mixture.
  1. Why is soil a heterogeneous mixture? (That is, what does it consist of?) ______
  1. FITB: In a ______mixture, the component particles cannot be distinguished.
  1. A homogeneous mixture is also called a ______.
  1. Examples of solutions …

Type of Solution / Solid / Liquid / Gas
Example

Matter and Atomic Structure Lesson 8

States of Matter

Name: ______Date: ______Period: _____

Notes:

Read and Draw: Read page 67-69.

A. FITB: Solids …

  1. A solid is a substance with densely ______particles.
  1. Most solids have a ______structure.
  1. Crystals form symmetrical solid objects with ______faces and ______edges between faces.
  1. A glass is a solid that consists of densely packed atoms arranged at ______. Glasses form when molten material is chilled so rapidly that atoms cannot arrange themselves into a regular ______.
  1. Draw the (solid) crystals of Figure 3-12 and write the caption.

Table Salt Crystals

/ Vanadium Crystals /

Caption

  1. FITB: Liquids …
  1. When the particles of a substance can slide past each other, the substance becomes ______.
  1. Liquids do not have their own ______but take the shape of the container they are placed in.
  1. Liquids do have a definite ______.

C . FITB: Gases …

  1. In gases, the particles are separated by relatively ______distances and move about at extremely ______speeds.
  1. Gases have no definite ______and no definite ______.
  1. Changes of State…
  2. What is melting? ______
  1. What is evaporation? ______
  1. What is sublimation? ______
  1. What is condensation? ______
  1. FITB: Plasma …

Plasma occurs when temperatures exceed ______degrees C. The collisions between particles are so violent that ______are knocked away from atoms. Three examples of plasma include: ______, ______, and ______.