Chpt 11. Lessons 2 & 3 quiz Physical Science JHS 8th Grade

Coach G or Mr. Giambelluca science 2nd quarter lesson 2 and 3 chapter 11 quizlet.

Ionic Bond

- Formed between oppositely charged ions.

Metallic Bond

- A bond formed by the attraction between positively charged metal ions and the electrons around them.

Properties of Metallic Bonds

- Electrons move freely between metal. - Conduct heat and electricity. - Metallic bonds are flexible.

Polyatomic Ion

An ion made of two or more atoms.

Common Polyatomic Ions

- There are many common polyatomic ions.

Parenthesis in Polyatomic Ion

- Parenthesis group the atoms of a polyatomic ion.

Polyatomic Ion Names and Oxygen Content

- Some polyatomic ion names relate to their oxygen content.

Know that the reason atoms bond is to become chemically stable.

Atoms bond to achieve chemical stability.

Atoms will gain/lose or share electrons so that they have more chemical stability.

To achieve chemical stability, atoms can either gain, lose, or share electrons.

Atoms with less than 8 valence electrons will try to combine (gain/lose electrons) with other chemical bonds/elements.

Atoms that have fewer than 8 valence electrons will attempt to gain or lose electrons by forming bonds with other elements.

A covalent bond forms when two nonmetal atoms share one or more pairs of valence electrons.

Covalent bonding occurs when two nonmetal atoms share valence electrons.

There could be single, double, or triple covalent bonds.

Covalent bonds can be single, double, or triple, depending on the number of electron pairs shared.

When two or more atoms share valence electrons, they form a stable covalent compound.

A stable covalent compound is formed when two or more atoms share valence electrons.

Covalent compounds have properties like low melting points, low boiling points, usually gases and liquids but can be solids at room temperature. They are poor conductors of thermal energy and electricity.

Covalent compounds typically have low melting and boiling points, are often in the form of gases or liquids, and are not good conductors of thermal energy or electricity.

Covalent compounds are made of molecules.

Molecules are the building blocks of covalent compounds.

A molecule is a group of atoms held together by covalent bonding that acts as an independent unit.

A molecule is a self-contained unit composed of atoms held together by covalent bonds.

Molecules are a chemically stable unit of a covalent compound.

Molecules represent the stable units within a covalent compound.

A covalent compound: A bond formed when atoms share one or more pairs of electrons.

A covalent compound is formed through the sharing of one or more pairs of electrons between atoms.

Bonds in which atoms share electrons equally are called Nonpolar covalent bonds.

When electrons are shared equally between atoms, the resulting bond is called a nonpolar covalent bond.

In nature, pure elements are rare.

Pure elements are not commonly found in nature.

Chemical bonds distinguish compounds from mixtures.

Chemical bonds are the defining feature that sets compounds apart from mixtures.

Atoms of different elements chemically combine to form compounds.

Compounds are created when atoms of different elements undergo chemical bonding.

A compound is held together by chemical bonds.

Chemical bonds are responsible for the cohesive forces that hold compounds together.

A chemical bond is the attractive force that holds two or more atoms or ions together.

Chemical bonds are the attractive forces that bind atoms or ions together.

The electrons that participate in chemical bonding.

Electrons are the particles involved in the process of chemical bonding.

Know the number of valence electrons for groups 1, 2, 13-18.

It is important to be aware of the number of valence electrons for elements in groups 1, 2, and 13-18.

Determining the number of valence electrons for groups 3-12 is more complicated.

Figuring out the number of valence electrons for elements in groups 3-12 requires a more complex approach.

American chemist Gilbert Lewis developed a method to show an element's valence electrons (Lewis dot diagram).

Gilbert Lewis, an American chemist, introduced the Lewis dot diagram as a way to represent the valence electrons of an element.