Chemistry Chapter: Ionic and Covalent Bonding

<p>By using the same name as the metal. (A)</p> Signup and view all the answers

<p>+1 (A)</p> Signup and view all the answers

<p>Anions are formed by gaining electrons. (B)</p> Signup and view all the answers

<p>They end with the suffix 'ide'. (A)</p> Signup and view all the answers

<p>They can have various charges needing Roman numerals. (B)</p> Signup and view all the answers

<p>Magnesium oxide (B)</p> Signup and view all the answers

<p>Ca3N2 (C)</p> Signup and view all the answers

<p>-2 (A)</p> Signup and view all the answers

<p>2 (C)</p> Signup and view all the answers

<p>With a Roman numeral (C)</p> Signup and view all the answers

<p>SO4^2- (D)</p> Signup and view all the answers

<p>NH4PO4 (C)</p> Signup and view all the answers

<p>Electrons are shared between atoms (B)</p> Signup and view all the answers

<p>Li1 F1 → LiF (A)</p> Signup and view all the answers

<p>K3N - Potassium nitride (C)</p> Signup and view all the answers

A chemical bond formed by the complete transfer of electrons from a metal to a non-metal, resulting in the formation of positively charged ions (cations) and negatively charged ions (anions). The electrostatic attraction between these oppositely charged ions forms the ionic bond.

A chemical compound formed by the electrostatic attraction between positively charged metal ions (cations) and negatively charged non-metal ions (anions).

The rule that states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight electrons in their outermost shell, like the noble gases.

A positively charged ion formed when an atom loses one or more electrons.

A negatively charged ion formed when an atom gains one or more electrons.

The smallest electrically neutral unit of an ionic compound, consisting of a specific ratio of cations and anions.

A system for naming and writing formulas for ionic compounds, based on the charges of the ions and the need for electrical neutrality.

Chemical compounds formed by the sharing of electrons between two non-metal atoms. Each atom contributes one or more electrons to the shared pair, forming a covalent bond.

A chemical bond formed by the sharing of one or more pairs of electrons between two non-metal atoms.

The process of assigning Roman numerals to the charge of a transition metal ion in an ionic compound.

A chemical bond formed by the electrostatic attraction between oppositely charged ions.

A group of elements in the periodic table that have a full outer shell of electrons and are very stable.

Elements found naturally on Earth.

A substance composed of two or more different elements chemically combined in a fixed ratio.

The chemical formula that represents the simplest whole-number ratio of atoms in a compound.

A neutral group of covalently bonded atoms.

Group 6 elements gain 2 electrons to achieve a full outer shell, resulting in a -2 charge. Think of it like filling a cup with 2 more electrons.

Elements in Group 5 seek stability by gaining 3 electrons to complete their outer shell, creating a -3 charge.

Polyatomic ions are groups of non-metals that act as a single, charged unit. They typically have a negative charge, which is why they are often called anions. Examples include sulfate (SO42-), hydroxide (OH-), and phosphate (PO43-),

To name an ionic compound, write the metal cation first, followed by the non-metal anion with an 'ide' ending. For instance, NaCl becomes sodium chloride, and MgO turns into magnesium oxide.

The formula of an ionic compound is determined by balancing the charges of the cation and anion in the lowest possible whole number ratio. For example, Lithium fluoride (Li+ and F-) results in LiF.

The ultimate switch-a-roo: the charge of one ion is the subscript for the other. This ensures a neutral formula unit. For instance, in calcium nitride (Ca+2 and N-3), the 2 charge of Ca is the subscript for N (N2), and the 3 charge of N is the subscript for Ca (Ca3), resulting in Ca3N2.

Transition metals often have multiple charges, which are indicated by Roman numerals in their names. For example, Manganese(IV) oxide means manganese has a +4 charge (Mn4+) and oxygen has a -2 charge (O2-), resulting in MnO2.

Molecular compounds are formed by two or more non-metals that share electrons to attain a full valence shell. They exist as molecules and do not involve ions. Examples: H2O, CO2, H2SO4.

Molecular compounds typically have low melting and boiling points and are often liquids or gases at room temperature. The atoms share electrons to reach a full valence shell, unlike ionic compounds where complete transfer of electrons occurs to form ions.

When naming compounds with transition metals (excluding groups 1A, 2A, and 3A), use Roman numerals to denote the charge of the metal. For example, Co2O becomes Cobalt (I) oxide, indicating a +1 charge on Cobalt.