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Questions and Answers
An ______ is the smallest particle that retains the chemical properties of an element.
An ______ is the smallest particle that retains the chemical properties of an element.
atom
A ______ is the smallest particle that retains the chemical properties of a compound.
A ______ is the smallest particle that retains the chemical properties of a compound.
molecule
Ionic bonds result from the ______ of electrons from one element to another.
Ionic bonds result from the ______ of electrons from one element to another.
transfer
______ are positively charged ions.
______ are positively charged ions.
Metals, like sodium (Na) and magnesium (Mg), form ______ by losing electrons.
Metals, like sodium (Na) and magnesium (Mg), form ______ by losing electrons.
Nonmetals, like chlorine (Cl), form ______ by gaining electrons.
Nonmetals, like chlorine (Cl), form ______ by gaining electrons.
Bonding is the joining of two atoms in a ______ arrangement.
Bonding is the joining of two atoms in a ______ arrangement.
Physical properties can be observed or measured without changing the composition of the material, such as ______ point.
Physical properties can be observed or measured without changing the composition of the material, such as ______ point.
A physical change alters the material without changing its ______.
A physical change alters the material without changing its ______.
Chemical properties determine how a substance can be converted into another substance through a ______.
Chemical properties determine how a substance can be converted into another substance through a ______.
A pure substance is composed of only a single ______ (atom or molecule).
A pure substance is composed of only a single ______ (atom or molecule).
A pure substance can be classified as an element or a ______.
A pure substance can be classified as an element or a ______.
Table sugar and water are both examples of ______ substances.
Table sugar and water are both examples of ______ substances.
Sugar dissolved in water is an example of a ______.
Sugar dissolved in water is an example of a ______.
Mixtures can be separated into their components by a ______ process.
Mixtures can be separated into their components by a ______ process.
An atom forms an anion with a completely filled outer shell of ______.
An atom forms an anion with a completely filled outer shell of ______.
The octet rule states that a main group element is especially stable when it possesses an octet of ______ in its outer shell.
The octet rule states that a main group element is especially stable when it possesses an octet of ______ in its outer shell.
The formula for calcium chloride is CaCl______
The formula for calcium chloride is CaCl______
The group number for metals in groups 1A, 2A, and 3A is equal to the charge on the ______.
The group number for metals in groups 1A, 2A, and 3A is equal to the charge on the ______.
Cations are named for the element from which they are formed, such as sodium (Na______) and potassium (K______).
Cations are named for the element from which they are formed, such as sodium (Na______) and potassium (K______).
For nonmetals in Groups 6A and 7A, the anion charge is calculated as ______ minus the group number.
For nonmetals in Groups 6A and 7A, the anion charge is calculated as ______ minus the group number.
An ionic bond is formed when a metal transfers one or more ______ to a nonmetal.
An ionic bond is formed when a metal transfers one or more ______ to a nonmetal.
Anions are named by replacing the ending of the element name by the suffix '-______'.
Anions are named by replacing the ending of the element name by the suffix '-______'.
The element symbol for chloride is Cl______.
The element symbol for chloride is Cl______.
In an ionic compound, the sum of the charges must be ______.
In an ionic compound, the sum of the charges must be ______.
To achieve a zero overall charge, subscripts are used to indicate the number of each ______.
To achieve a zero overall charge, subscripts are used to indicate the number of each ______.
To write a formula for an ionic compound, it is important to identify which element is the ______ and which is the anion.
To write a formula for an ionic compound, it is important to identify which element is the ______ and which is the anion.
The main group cation for magnesium is Mg______.
The main group cation for magnesium is Mg______.
When the cation and anion have the same charge, only ______ of each is needed to achieve a zero charge.
When the cation and anion have the same charge, only ______ of each is needed to achieve a zero charge.
For an ionic compound, the cation is placed ______ and the anion is placed second in the formula.
For an ionic compound, the cation is placed ______ and the anion is placed second in the formula.
Examples of ionic compounds include KCl, CaO, and CaCl______.
Examples of ionic compounds include KCl, CaO, and CaCl______.
Covalent bonds result from the sharing of ______ between two atoms.
Covalent bonds result from the sharing of ______ between two atoms.
A molecule is a discrete group of ______ held together by covalent bonds.
A molecule is a discrete group of ______ held together by covalent bonds.
Unshared electron pairs are called ______ electron pairs.
Unshared electron pairs are called ______ electron pairs.
Lewis structures are electron-dot structures that show the location of all ______ electrons.
Lewis structures are electron-dot structures that show the location of all ______ electrons.
A double bond contains ______ electrons in two bonds.
A double bond contains ______ electrons in two bonds.
The first step in naming a covalent molecule is to name the first ______ by its element name.
The first step in naming a covalent molecule is to name the first ______ by its element name.
When naming the second element, you use the suffix '[-blank]'.
When naming the second element, you use the suffix '[-blank]'.
Add ______ to show the number of atoms of each element in a covalent compound.
Add ______ to show the number of atoms of each element in a covalent compound.
The prefix 'mono' indicates ______ atom.
The prefix 'mono' indicates ______ atom.
The chemical formula for nitrogen dioxide is ______.
The chemical formula for nitrogen dioxide is ______.
In a balanced chemical equation, the number of atoms of each element must be equal on both the ______ and the product side.
In a balanced chemical equation, the number of atoms of each element must be equal on both the ______ and the product side.
Carbon monoxide consists of one atom of carbon attached to one atom of ______.
Carbon monoxide consists of one atom of carbon attached to one atom of ______.
The chemical formula for carbon dioxide is ______.
The chemical formula for carbon dioxide is ______.
Oxidation/reduction reactions involve the transfer of ______ from one atom to another.
Oxidation/reduction reactions involve the transfer of ______ from one atom to another.
The prefix 'di' indicates ______ atoms in a chemical compound.
The prefix 'di' indicates ______ atoms in a chemical compound.
The reaction type where one element replaces another in a compound is called ______ replacement.
The reaction type where one element replaces another in a compound is called ______ replacement.
Flashcards
Pure Substance
Pure Substance
A material composed of only one type of atom (element) or molecule (compound).
Element
Element
A pure substance that cannot be broken down into simpler substances by chemical means.
Compound
Compound
A pure substance formed when two or more elements chemically combine in a fixed ratio.
Mixture
Mixture
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Physical Change
Physical Change
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Physical Property
Physical Property
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Chemical Property
Chemical Property
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Chemical Change
Chemical Change
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Atom
Atom
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Molecule
Molecule
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Ionic Bond
Ionic Bond
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Covalent Bond
Covalent Bond
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Cation
Cation
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Anion
Anion
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Electron Configuration
Electron Configuration
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Noble Gas
Noble Gas
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Octet rule
Octet rule
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Anion formation
Anion formation
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Cation charge
Cation charge
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Anion charge
Anion charge
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Ionic compound
Ionic compound
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Identifying cation/anion in formula
Identifying cation/anion in formula
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Ionic compound formula
Ionic compound formula
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Cation Naming (Main group)
Cation Naming (Main group)
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Anion Naming
Anion Naming
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Ionic Formula - Balancing Charges
Ionic Formula - Balancing Charges
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Example Ionic Compound - KCl
Example Ionic Compound - KCl
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Example Ionic Compound - CaCl2
Example Ionic Compound - CaCl2
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Subscript in Formula
Subscript in Formula
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Naming Ionic Compound (Steps)
Naming Ionic Compound (Steps)
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Mono, Di, Tri, etc.
Mono, Di, Tri, etc.
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Covalent Compound Naming
Covalent Compound Naming
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Chemical Equation
Chemical Equation
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Balanced Chemical Equation
Balanced Chemical Equation
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Reactants
Reactants
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Products
Products
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Oxidation/Reduction (Redox) Reaction
Oxidation/Reduction (Redox) Reaction
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Types of Reactions
Types of Reactions
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Lewis Structures
Lewis Structures
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Double Bond
Double Bond
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Triple Bond
Triple Bond
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Valence Electrons
Valence Electrons
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Naming Covalent Compounds - Steps
Naming Covalent Compounds - Steps
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Unshared Electron Pairs
Unshared Electron Pairs
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Study Notes
Physical Properties of Matter
- Physical properties describe a substance without changing its composition
- Examples include boiling point, melting point, solubility, color, and odor.
Physical Changes
- A physical change alters a material's form, but not its composition.
- Examples include melting, boiling, and dissolving.
Chemical Properties of Matter
- Chemical properties describe how a substance can be converted into a different substance.
- Chemical properties determine how a substance reacts with other substances
- Examples of chemical properties include flammability.
Chemical Changes
- A chemical change results in a new substance(s) with different properties.
- Occurs through chemical reactions converting one substance into another(s)
- Examples of chemical changes are combustion, rusting, corrosion, and oxidation
Classification of Matter
- All matter is either a pure substance or a mixture
- Pure Substances:
- Composed of only one type of component (atom or molecule).
- Have a constant composition regardless of the sample size or origin.
- Cannot be broken down into simpler substances through physical changes.
- Can be an element or compound.
Elements
- Pure substances that cannot be broken down into simpler substances by chemical changes.
- Examples: aluminum foil, nitrogen gas.
Compounds
- Pure substances formed by chemically joining two or more elements.
- Examples: water (Hâ‚‚O), table salt (NaCl).
Mixtures
- Composed of more than one component.
- Have varying compositions (combinations of solid, liquid, and gas).
- Can be separated physically.
- Examples: sugar dissolved in water.
Atoms and Molecules
- Atoms: smallest particles with chemical properties of an element
- Molecules: smallest particle with the chemical properties of a compound.
- Examples:
- Diatomic molecules: oxygen (Oâ‚‚), hydrogen (Hâ‚‚)
- Triatomic molecule: ozone (O₃)
- Examples:
lonic Bonding
- Forms between a metal and a nonmetal.
- Results from the transfer of electrons.
- The sum of the charges in an ionic compound must equal zero.
Ions
- Charged species.
- Cations: positively charged
- Anions: negatively charged
Ionic Compounds
- Formed by the electrostatic attraction between cations and anions.
- The sum of the charges in an ionic compound must be zero overall.
- Names consist of the cation (+), then anion (-).
- Examples:
- NaCl (sodium chloride)
- CaO (calcium oxide)
Covalent Bonding
- Results from the sharing of electrons.
- Bonds between nonmetals.
- A molecule is formed when atoms bond covalently
Lewis Structures
- Electron-dot structures of molecules.
- Shows valence electrons.
Multiple Bonds
- Covalent bonds can be single, double, or triple.
- Double bond: shares four electrons
- Triple bond: shares six electrons
Naming Covalent Compounds
- Name first element with prefix designating number of atoms, then name second element with appropriate prefix and suffix "-ide."
- Prefixes (from Table 4.1):
- Mono- (1) / Di- (2) / Tri- (3) / Tetra- (4) / Penta- (5) / Hexa- (6) / Hepta- (7) / Octa- (8)/ Nona- (9) / Deca- (10)
Chemical Equations
- Represent chemical reactions using chemical symbols and formulas.
- Reactants are shown on the left, and products are shown on the right.
- The arrow signifies the change
Types of Reactions
- Combination: two or more reactants combined to form one product
- Decomposition: one reactant broken down to form two or more products
- Single replacement: one element replaces another element in a compound
- Double replacement: two compounds exchange parts (atoms or ions)
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Description
Test your knowledge on the physical and chemical properties of matter with this quiz. Understand the differences between physical changes and chemical changes, and learn how to classify matter. This quiz covers key concepts surrounding the composition and transformation of substances.
