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Questions and Answers
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.
Questions and Answers
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Flashcards
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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Flashcards
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Study Notes
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 (H₂O), 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 (O₂), hydrogen (H₂)
- 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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