Atoms and Elements

Unit on how to describe, catagorize, and locate elements and compounds using the periodic table.

List and explain two WHIMIS symbols?

Flashcard #1
Term: What does WHMIS stand for?
Definition: WHMIS stands for Workplace Hazardous Materials Information System.

Flashcard #2
Term: What does the Flame pictogram indicate?
Definition: The Flame pictogram indicates that a product is flammable (e.g., gases, aerosols, liquids, solids), pyrophoric (catches fire spontaneously), or self-heating.

Divide Matter into its two broad categories and sub-categories.

Matter Flow Chart:

1. Matter

   • Pure Substances

     • Elements

     • Compounds

   • Mixtures

     • Homogeneous Mixtures

     • Heterogeneous Mixtures

Name 4 physcial properties of elements?

Definition: Four physical properties of elements include:

1. Melting Point: The temperature at which an element changes from a solid to a liquid.

2. Boiling Point: The temperature at which an element changes from a liquid to a gas.

3. Density: The mass of an element per unit volume.

4. Electrical Conductivity: The ability of an element to conduct electric current.

Name 4 chemical properties

Definition: Definition: Four chemical properties of elements include:

1. Reactivity: How readily an element undergoes a chemical reaction with other substances (e.g., oxygen, water, acids, bases).

2. Flammability: The ability of an element to burn or ignite, causing fire or combustion.

3. Oxidation/Corrosion: The tendency of an element to react with oxidizers (like oxygen) leading to the formation of oxides or other degraded products (e.g., rusting of iron).

4. Toxicity: The inherent ability of an element to cause harm to living organisms.

What is the difference between Chemical and Physical properties of elemements?

• Physical Properties: Can be observed or measured without changing the chemical identity of the substance (e.g., melting point, density).

• Chemical Properties: Describe how a substance reacts to form new substances, which changes its chemical identity (e.g., flammability, reactivity).

List the three major categories in the periodic table and breifly describe them.

• Metals:

  • Typically solid at room temperature (except Mercury).

  • Good conductors of heat and electricity.

  • Malleable (can be hammered into sheets) and ductile (can be drawn into wires).

  • Lustrous (shiny).

• Nonmetals:

  • Can be solid, liquid, or gas at room temperature.

  • Generally poor conductors of heat and electricity (insulators).

  • Brittle in solid form.

  • Not lustrous.

• Metalloids:

  • Have properties intermediate between metals and nonmetals.

  • Often semiconductors (can conduct electricity under certain conditions).

  • Examples include Boron, Silicon, and Germanium.

Name and describe the two type of bonds that occur to create compounds?

Definition: - Ionic Bonds:
- Involve the transfer of electrons from a metal to a nonmetal.
- Results in oppositely charged ions that attract each other.
- Example: Sodium chloride (NaCl), where NaNa loses an electron to ClCl to form Na+Na+ and Cl−Cl− ions.

• Covalent Bonds:

  • Involve the sharing of electrons between two nonmetal atoms.

  • Creates strong bonds that form molecules.

  • Example: Water (H2OH2​O), where oxygen shares electrons with two hydrogen atoms.

Give a brief explanation of Akaline, Alkali metals as well as the noble gases?

Alkali Metals:
- Found in Group 1 of the periodic table (e.g., Sodium, Potassium).
- They are very reactive metals, especially with water.
- Have 1 electron in their outermost shell, which they easily lose.

• Alkaline Earth Metals:

  • Found in Group 2 of the periodic table (e.g., Magnesium, Calcium).

  • They are reactive metals, but less so than alkali metals.

  • Have 2 electrons in their outermost shell.

• Noble Gases:

  • Found in Group 18 of the periodic table (e.g., Neon, Argon).

  • They are very unreactive (inert) gases.

  • Have a full outermost electron shell (usually 8 electrons), making them very stable and unlikely to form compounds.

Create a Bohr Diagram

Here's how to create one:

1. Nucleus: Draw a central circle representing the nucleus. Inside, write the number of protons (p+p+) and neutrons (n0n0).

2. Electron Shells: Draw concentric circles around the nucleus to represent the electron shells or energy levels.

3. Place Electrons: Distribute the electrons (as dots or 'x's) onto these shells, starting from the innermost shell, following these rules:

   • The first shell can hold a maximum of 22 electrons.

   • The second shell can hold a maximum of 88 electrons.

   • Always fill an inner shell completely before moving to the next outer shell.

Example: For an Oxygen atom (with 88 protons, 88 neutrons, and 88 electrons):

• Nucleus: 8p+8p+, 8n08n0

• First shell: 22 electrons

• Second shell: 66 electrons (since 88 total electrons - 22 in the first shell = 66 remaining).