Sci 10 Chem Quiz

Quiz Date: Monday, October 5 2026

Atomic Theory: Atom

Smallest particle of an element

Atomic Theory: 3 subatomic particles (smaller particles atoms are made of)

Protons, neutrons, & electrons

Atomic Theory: Charges of 3 subatomic particles

Protons: postitive

Neutrons: no electric charge/ neutral

Electrons: negative

Atomic Theory: Subatomic particles all have __

Subatomic particles have mass, but protons & electrons have electric charge

Atomic Theory: Location of 3 subatomic particles

Nucleus (central part of atom where most mass is found) = Protons + Neutrons

→ nuclear charge is always positive

→ particles are tightly packed in the centre of atom — mass of proton & neutron = 1 atomic mass unit (amu)

Outside the Nucleus = Electrons — circle nucleus very quickly

→ electrons are light & have mass of 1/1800 amu/almost no mass

Atomic Theory: # of protons are equal to (periodic table)

Number of protons = atomic number (for neutral atoms also = number of electrons)

Atomic Theory: Difference between mass number & atomic mass

Mass number = whole number/rounded of amu

Atomic mass = mass of average atom (on periodic table)

Atomic Theory: Difference between ion & atom

Ion = electric charge that forms when atom gain/loses electrons — unequal # of protons & electrons

Atom = neutrally charged, same # of protons & electron

Atomic Theory: How to find # of neutrons

Neutrons = mass number - protons

Atomic Theory: Location of metals, non-metals. & metalloids

Metals = left side & middle of table (more conductive)

Non-metals = upper right corner (yellow)

Metalloids = form staircase toward the right side (pink)

Atomic Theory: Names for Group 1, 2, 17, 18, 3-12

Group 1 - Alkali metals

Group 2 - Alkaline earth metals

Group 17 - Halogens

Group 18 - Noble gases

Group 3-12 - Transition metals

Atomic Theory: Difference between group & period

Group = column in periodic table

Period = row in periodic table

Atomic Theory: Another term for group

Group is also known as “Family”

Atomic Theory: Difference between cation & anion

Cation = + positivity charged ions (metals lose e-)

Anion = - negatively charged ions (non-metals gain e-)

Atomic Theory: Difference between an ion w/ 2+ & ion w/ 2-

Ion w/ 2+ - metal element that loses 2 electrons

Ion w/ 2- - non-metal element that gains 2 electrons

Atomic Theory: How many electrons does an ion w/ 3+ have & ion w/ 3-

Ion w/ 3+ - Protons > electrons (e.g. e = p - 3)

Ion w/ 3- - Electrons > protons (e.g. e = p + 3)

Atomic Theory: What does periodic table show?

Elements w/ similar properties have similar electron arrangement

Bohr Model: What does Bohr model show?

Electron arrangement in shells

Bohr Model: Name of the outermost shell

Valence shell (electrons = valence electrons)

Bohr Model: Other terms for electron shells

Orbits, energy levels

Bohr Model: Maximum # of electrons each electron shell hold

First shell - 2 electrons

Second shell - 8 electrons

Third shell - 8 electrons

**Fourth shell - 18 electrons

Bohr Model: Chemical name for NH3, CH4, and H2O

NH3 = ammonia

CH4 = methane

H2O = water

Bonding: 2 differences between ionic & covalent bonding

Ionic bonding:

→ ionic compound has positive (metal) & negative (non-metal) ion

→ 1 or more electrons transfer from metal to non-metal

Covalent bonding:

→ formed between two or more non-metals

→ electrons shared between atoms

Covalent Bonding: Difference between bonding pair & lone pair

Bonding pair = shared pair of electrons

Lone pair = pair of electrons in the valence shell not used in bonding

Bonding/Diagram: What type of bond & diagram can we use a line to represent a pair of electrons?

Type of bond: covalent bonds

Diagram: Lewis diagram

Diagrams: Differences between Bohr model & Lewis diagram

Bohr Model:

→ diagram shows # of electrons in each of the energy levels/electron shells around an atom

Lewis Diagram:

→ diagram the shows chemical bonding drawing ONLY atom’s valence electrons & chemical symbol

→ drawn w/ dots (electrons) placed around the element symbol (N,E,S,W)

Lewis Diagram: What rule do we need to follow when we draw Lewis Diagram?

Octet Rule = Most atoms want 8 valence electrons to be stable

Elements/Ions: What of the following have the same energy levels: Mg2+, F, & Ar

Mg2+ & F

→ Mg has 3 electron shells, but loses 2 electrons making it have 2 electron shells/energy levels

→ F has 2 energy levels/electron shells

Ar has 3 energy levels/electron shells

Elements: 7 Diatomic Particles

Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (Cl2), Bromine (Br2), Iodine (I2)

Ways to Remember:

HOFBrINCl

Number 7 on periodic table

Naming Compounds: When do we use Roman numerals?

Use Roman numerals for multivalent compounds

Naming Compounds: When can we use prefixes?

Use prefixes for covalent compounds

Naming Compounds: When do we have to add brackets when we write chemical formulae?

Polyatomic ions when you criss-cross, # of ion is greater than 1 — add brackets

Naming Compounds: What situation(s) that we cannot reduce the subscripts?

Covalent compounds or if you cannot divide an ionic/polyatomic compound subscripts of both ions with the same #