Science 10: Periodic Table, Atomic Theory, and Chemical Compounds

Comprehensive vocabulary flashcards covering the periodic table organization, atomic structure, Bohr models, valence electrons, ions, ionic and covalent bonding, polyatomic ions, and acid nomenclature based on the Science 10 chemistry notes.

Periodic Table

A chart that organizes the elements according to their physical and chemical properties.

Period

A horizontal row of elements in the periodic table; there are $7$ periods in total, and the period number equals the number of occupied electron shells in an atom.

Chemical Family (Group)

A vertical column in the periodic table ($18$ in total) containing elements that share similar physical and chemical properties and have the same number of valence electrons.

Metals

Elements positioned on the left and centre of the periodic table that are generally good conductors of heat and electricity, reactive, and tend to lose electrons to form positive ions.

Non-metals

Elements positioned on the right side of the periodic table that are poor conductors of heat and electricity and tend to gain electrons to form negative ions.

Metalloids

Elements arranged in a zigzag staircase pattern toward the right side of the periodic table (such as boron and silicon) that have properties of both metals and non-metals.

Alkali Metals

Group $1$ metallic elements (excluding hydrogen) that are strongly reactive, soft, have low densities, and form ions with a $+1$ charge by giving away $1$ electron.

Alkaline Earth Metals

Group $2$ metallic elements (including beryllium and magnesium) that are reactive, fairly soft, have fairly low densities, and give away $2$ electrons to form ions with a $+2$ charge.

Halogens

Group $17$ non-metallic elements that are strongly reactive, have $7$ valence electrons, take $1$ electron to form ions with a $-1$ charge, and exist as gases at room temperature (except bromine, which is a liquid).

Noble Gases

Group $18$ non-metallic elements that are extremely unreactive, colourless, odourless gases at room temperature with completely filled valence shells ($8$ valence electrons, except helium which has $2$).

Atomic Number

The specific number of protons found in the nucleus of each atom of an element, which also equals the number of electrons in a neutral atom.

Average Atomic Mass

The weighted average of the masses of the naturally occurring isotopes of an element, based on the mass of carbon-12 at exactly $12.00$.

Number of Neutrons Calculation

The formula used to determine neutrons in an atom: $\text{Atomic Mass} - \text{Atomic Number} = \text{Number of Neutrons}$ (for example, in titanium: $48 - 22 = 26$).

Ion Charge

The electric charge that forms on an atom when it either gains or loses electrons; calculated as the sum of the charges of its protons and electrons.

Multiple Ion Charge

The capacity of certain transition metals (such as titanium, cobalt, and platinum) to form ions in more than one way with different electric charges.

Bohr Model

A diagram that displays the number and arrangement of electrons in each energy level or electron shell around an atom's nucleus.

Electron Shell Capacities

The maximum number of electrons that can occupy each successive energy level: shell 1 holds $2$, shell 2 holds $8$, shell 3 holds $8$, shell 4 holds $18$, shell 5 holds $18$, and shell 6 holds $32$.

Valence Shell

The outermost occupied electron shell of an atom that holds the electrons located farthest away from the nucleus.

Valence Electrons

The electrons located exclusively in the outermost energy level (valence shell) of an atom.

Ion

An electrically charged atom formed when a neutral atom gains electrons (forming a negatively charged ion) or loses electrons (forming a positively charged ion).

Element

A pure chemical substance that is composed entirely of one single type of atom.

Compound

A pure substance composed of two or more different types of atoms chemically bonded together through a chemical change.

Chemical Bond

Attractive electrostatic forces that hold atoms together in molecules or ions in crystal lattices, formed by transferring or sharing electrons.

Ionic Compound

A compound formed between a metal and a non-metal when electrons are transferred from the metal to the non-metal, producing oppositely charged ions that balance to create an overall neutral compound.

Ionic Lattice

A repeating three-dimensional pattern of alternating positive and negative ions held together by ionic bonds in a solid ionic compound.

Covalent Compound

A compound formed when two or more non-metal atoms combine by sharing valence electrons rather than gaining or losing them.

Molecule

An electrically neutral group of two or more non-metal atoms joined together by covalent bonds.

Polyatomic Ion

A charged chemical unit consisting of two or more atoms that are held together internally by covalent bonds but carry an overall net electrical charge.

Diatomic Elements

Seven elements that naturally pair as two-atom molecules and never exist as isolated single atoms: $H_2, N_2, O_2, F_2, Cl_2, Br_2, I_2$.

Ammonium Ion

A positively charged polyatomic ion with the chemical formula $NH_4^+$ and a charge of $+1$.

Nitrate Ion

A polyatomic ion composed of nitrogen and oxygen with the formula $NO_3^-$ and an overall charge of $-1$.

Hydroxide Ion

A polyatomic anion with the formula $OH^-$ and an electric charge of $-1$.

Carbonate Ion

A polyatomic anion composed of carbon and oxygen with the formula $CO_3^{2-}$ and an electric charge of $-2$.

Sulfate Ion

A polyatomic anion composed of sulfur and oxygen with the formula $SO_4^{2-}$ and an electric charge of $-2$.

Phosphate Ion

A polyatomic anion composed of phosphorus and oxygen with the chemical formula $PO_4^{3-}$ and an electric charge of $-3$.

Common Acids

Key acids specified on the data sheet: Hydrochloric acid ($HCl$), Sulfuric acid ($H_2SO_4$), Nitric acid ($HNO_3$), and Acetic acid ($HCH_3COO$).

Acid Naming Rule: -ide

A naming rule stating that an anion ending in '-ide' forms an acid named with the prefix 'hydro-' and suffix '-ic acid' (e.g., chloride becomes hydrochloric acid).

Acid Naming Rule: -ate

A naming rule stating that a polyatomic anion ending in '-ate' forms an acid ending in '-ic acid' (e.g., nitrate becomes nitric acid).

Acid Naming Rule: -ite

A naming rule stating that a polyatomic anion ending in '-ite' forms an acid ending in '-ous acid' (e.g., nitrite becomes nitrous acid).

Covalent Prefixes

Prefixes used to designate the number of atoms: mono- ($1$), di- ($2$), tri- ($3$), tetra- ($4$), penta- ($5$), hexa- ($6$), hepta- ($7$), octa- ($8$), nona- ($9$), deca- ($10$).

Metal Oxide Reaction

The reaction of a metal oxide with water to yield a basic hydroxide solution: $\text{metal oxide} + H_2O \rightarrow \text{base (hydroxide)}$.

Non-metal Oxide Reaction

The reaction of a non-metal oxide with water to produce an acid: $\text{non-metal oxide} + H_2O \rightarrow \text{acid}$.