Ionic & Covalent compounds
Metals and nonmetals form…
ionic compounds
The difference between a single bond, a double bond, and a triple bond is...
A single bond shares one pair of electrons, a double bond shares two pairs of electrons, and a triple bond shares three pairs of electrons.
Ex. Single bond: H₂ /Double bond: O₂ /Triple bond: N₂.
The definition of an ATOM & an example of one (H₂O) is...
The smallest unit of an element consists of protons, neutrons, and electrons.
Ex. A single hydrogen (H) atom
DRAW the Lewis Dot Diagram for Hydrogen!
A single dot representing one valence electron.
Metals form (1), Nonmetals form (2)
1. cations (positive)
2. anions (negative)
The three steps to writing the chemical formula of an ionic compound are...
Look at the compound's name to find the elements involved.
Use prefixes to determine the number of atoms for each element (mono-, di-, tri-, etc.).
Write the chemical symbols of the elements and add subscripts based on the prefixes.
Ex. "Carbon dioxide" → CO₂
The definition of a MOLECULE & an example of one (H₂O) is...
A group of two or more atoms bonded together.
Ex. Water (H₂O) is a molecule made of two hydrogen atoms and one oxygen atom covalently bonded.
DRAW the Lewis Dot Diagram for Carbon!
Four dots, evenly spaced around the "C," one on each side.
Nonmetals and metalloids (elements that are between metals and nonmetals) form (1) This happens when these elements (2) bond.
1. covalent compounds
2. share electrons
The three steps to name binary covalent compounds from their formulas are...
Identify the elements in the formula.
Count the atoms of each element.
Use prefixes to write the name (mono-, di-, tri-, etc.).
Ex. N₂O₄ → "Dinitrogen tetroxide"
The difference between an atom and a molecule is...
An atom is the smallest unit of an element, while a molecule is a group of two or more atoms bonded together.
DRAW the Lewis Dot Diagram for Nitrogen!
Five dots, a pair on one side, and single dots on the other three sides.
Covalent compounds are made when (1) share electrons to form a stable bond.
1. two or more nonmetals
The Lewis structure depicts (1) and total valence electrons are calculated by (2).
1. the arrangement of valence electrons in a molecule
2. adding the valence electrons of all atoms in the molecule.
Which rule explains how atoms gain, lose, or share electrons to achieve a stable outer shell of 8 electrons, resembling the electron configuration of noble gases?
The Octet rule.
DRAW the Lewis Dot Diagram for Oxygen!
Six dots, two pairs on two sides, and single dots on the remaining two sides.
A Covalent Bond is…
The bond formed when two atoms share electrons.
Covalent bonding electrons are (1) while lone electron pairs are (2).
1. shared between atoms to form bonds
2. non-bonding electrons localized on an atom.
How do atoms combine to form a covalent molecule?
By sharing electrons to achieve stable electron configurations, typically filling their outer shells.
DRAW the Lewis Dot Diagram for Fluorine!
Seven dots, three pairs, and one single dot.