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Questions and Answers
What kind of bond exists between the atoms of a diamond?
What kind of bond exists between the atoms of a diamond?
Which of the following will dissolve in a solution?
Which of the following will dissolve in a solution?
Which of the following substances has the weakest bonds?
Which of the following substances has the weakest bonds?
What is the main reason why sugar melts at a lower temperature compared to diamonds?
What is the main reason why sugar melts at a lower temperature compared to diamonds?
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What is the formula for calculating molarity?
What is the formula for calculating molarity?
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When calculating molarity, which of the following units must be converted to liters?
When calculating molarity, which of the following units must be converted to liters?
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When calculating molarity, what two pieces of information are required?
When calculating molarity, what two pieces of information are required?
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Which of the following is NOT a network covalent solid?
Which of the following is NOT a network covalent solid?
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Which of the following is NOT a characteristic of a polar molecule?
Which of the following is NOT a characteristic of a polar molecule?
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Which of the following is an example of a chemical change?
Which of the following is an example of a chemical change?
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Which type of bond involves the sharing of electrons?
Which type of bond involves the sharing of electrons?
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Which of the following is a characteristic of a solution?
Which of the following is a characteristic of a solution?
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Which of the following is NOT a characteristic of an ionic compound?
Which of the following is NOT a characteristic of an ionic compound?
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Which of the following is the correct order of bond strength, from weakest to strongest?
Which of the following is the correct order of bond strength, from weakest to strongest?
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Which of the following elements is most likely to form a cation?
Which of the following elements is most likely to form a cation?
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Which of the following is TRUE regarding London dispersion forces?
Which of the following is TRUE regarding London dispersion forces?
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Which of the following substances is most likely to dissolve in water?
Which of the following substances is most likely to dissolve in water?
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What is the mass number of an atom that has 17 protons and 18 neutrons?
What is the mass number of an atom that has 17 protons and 18 neutrons?
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Which of the following is NOT a characteristic of a heterogeneous mixture?
Which of the following is NOT a characteristic of a heterogeneous mixture?
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Which of the following best describes the relationship between concentration and solubility?
Which of the following best describes the relationship between concentration and solubility?
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Which of the following best describes the role of electrons in chemical bonding?
Which of the following best describes the role of electrons in chemical bonding?
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Which of the following statements best describes the relationship between electronegativity and bond type?
Which of the following statements best describes the relationship between electronegativity and bond type?
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What is the formula for calculating the number of moles of a substance, given its mass and molar mass?
What is the formula for calculating the number of moles of a substance, given its mass and molar mass?
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Which of the following is a polyatomic ion?
Which of the following is a polyatomic ion?
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Flashcards
Molarity
Molarity
Concentration of a solution measured in moles of solute per liter of solution.
Convert grams to moles
Convert grams to moles
Use the molar mass of a substance to convert grams into moles.
Covalent Bonds
Covalent Bonds
Strong bonds formed by the sharing of electrons between atoms, typical in diamond.
Intermolecular Forces
Intermolecular Forces
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Ionic Bonds
Ionic Bonds
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Melting Points and Bond Strength
Melting Points and Bond Strength
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Network Covalent Solids
Network Covalent Solids
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Polarity of Molecules
Polarity of Molecules
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Polar Molecule
Polar Molecule
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Hydrogen Bonding
Hydrogen Bonding
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London Dispersion Forces
London Dispersion Forces
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Solubility Rule
Solubility Rule
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Ionic Compounds in Water
Ionic Compounds in Water
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Concentration
Concentration
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Independent Variable
Independent Variable
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Dependent Variable
Dependent Variable
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Mass Number
Mass Number
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Avogadro's Number
Avogadro's Number
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Valence Electrons
Valence Electrons
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Octet Rule
Octet Rule
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Cation vs Anion
Cation vs Anion
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Electronegativity
Electronegativity
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Polyatomic Ion
Polyatomic Ion
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Study Notes
Molarity Calculations
- Molarity is calculated by dividing moles of solute by liters of solution.
- To calculate molarity, you need two values: moles of solute (grams or moles) and liters of solution (or any volume measurement in milliliters or centiliters, which must be converted to liters).
- To find liters, you need molarity and moles.
- To find moles, you need molarity and liters.
- Remember to convert units (e.g., milliliters to liters) as needed.
- Use molar mass to convert grams to moles.
Properties of Solids and Bonds
- Melting points are indicators of bond strength. Stronger bonds lead to higher melting points.
- Covalent bonds are extremely strong, as seen in diamonds.
- Diamonds melt at exceptionally high temperatures (7000°C) due to strong covalent bonds.
- Network covalent solids (diamond, graphite, sand) are strong due to the network of covalent bonds within these structures. Sand, although a molecule, is incredibly strong because of these internal bonds.
- Ionic bonds (e.g., NaCl) are strong but weaker than covalent bonds in network structures. These bonds melt at roughly 800°C.
- Metallic bonds are strong and result in high melting points. Metals are held together by a "sea of electrons."
- Intermolecular forces (forces between molecules) are weaker than intramolecular forces (e.g., covalent bonds within a molecule). Melting or boiling of covalent molecular compounds (like water or sugar) breaks the intermolecular bonds, not the covalent ones.
Types of Solids
- Ionic compounds and molecular compounds dissolve in solutions.
- Network covalent solids and metallic solids do not dissolve in solutions.
Intermolecular vs. Intramolecular Forces
- Intramolecular forces are forces within a molecule (e.g., covalent bonds).
- Intermolecular forces are forces between molecules (e.g., London Dispersion forces).
Polarity of Molecules
- Nonpolar molecules have atoms that are the same, or have even distributions of atoms around the central atom. These are held together by London Dispersion forces.
- Polar molecules are asymmetrical and have partial charges, leading to stronger intermolecular forces compared to nonpolar molecules.
- Superpolar molecules (hydrogen bonding) involve polar molecules with hydrogen bonded to highly electronegative atoms (fluorine, oxygen, or nitrogen). Hydrogen bonds are nearly as strong as ionic bonds.
- Order of bond strength (strongest to weakest): Ionic, Hydrogen Bonding, Polar Covalent, Nonpolar Covalent
Hydrocarbons
- Hydrocarbons are molecules composed of carbon and hydrogen.
- The state of a hydrocarbon at room temperature depends on its size: smaller hydrocarbons are gases, larger ones are liquids.
London Dispersion Forces (LDF)
- London Dispersion Forces occur in nonpolar molecules due to temporary shifts in electron distribution, creating temporary positive and negative charges that attract each other.
Solutions and Solubility
- For a solution to form, the solute (substance being dissolved) must be attracted to the solvent (substance doing the dissolving).
- Polar solutes dissolve in polar solvents.
- Nonpolar solutes do not dissolve in polar solvents.
- Ionic compounds dissolve in polar solvents (e.g., water).
- Solutes dissolve in solvents when the attraction between them is strong.
- Ionic, polar, and nonpolar substances dissolve according to the polarity of the molecules.
Ionic Solutes in Water
- Water dissolves ionic substances. The negative side of water (oxygen) aligns with positive ions. The positive side of water (hydrogen) aligns with negative ions. This strong attraction pulls the ionic substance apart.
Polar Solutes in Water
- Water dissolves polar substances in a manner similar to ionic substances by aligning the positive and negative parts of the water molecules with the opposite charges in the polar molecule.
Nonpolar Solutes in Water
- Water does not dissolve nonpolar substances due to a lack of attraction between the solute and solvent.
Concentration
- Concentration is the amount of solute in a given volume of solution.
- Concentration can be measured using numbers (quantitative data) and/or observations (qualitative data)
Scientific Notation and Significant Figures
- Scientific notation format: 860000 = 8.6 x 10^5
- Rules for significant figures: non-zeros are significant; zeros between non-zeros are significant; zeros after a non-zero after a decimal are significant. Exact numbers have infinite significant figures.
Basic Chemistry
- Atom: basic unit of an element.
- Element: composed of one type of atom.
- Molecule: two or more atoms bonded together (can be the same or different).
- Compound: two or more different types of atoms chemically bonded.
- Mixture: two or more different substances physically combined.
- Pure substance: has the same composition throughout.
- Heterogeneous: not uniform in composition.
- Homogeneous: uniform in composition.
- Quantitative data: data involving numbers.
- Qualitative data: data involving observations.
- Percent Error: a measure of agreement between the expected and experimental values.
Calculations and Variables
- Volume: Mass ÷ Density
- Mass: Moles × Molar Mass
- Density: Mass ÷ Volume
- Independent Variable: the variable that is changed.
- Dependent Variable: the variable that is measured.
- Control: the variable that remains constant.
Atomic Structure
- Atom: the smallest particle of an element.
- Atomic number: number of protons in an atom.
- Mass number: total number of protons and neutrons in an atom.
- Molar mass: the mass of one mole of a substance.
- Proton: positively charged particle within the nucleus.
- Neutron: neutrally charged particle within the nucleus.
- Electron: negatively charged particle outside the nucleus.
- Isotopes: atoms of the same element with different numbers of neutrons.
- Avogadro's number: 6.022 x 1023
Conversions
- Grams to Moles: Grams ÷ Molar Mass
- Moles to Grams: Moles × Molar Mass
- Molecules/Atoms to Moles: Given # ÷ Avogadro's Number
- Moles to Molecules/Atoms: Given # × Avogadro's Number
Periodic Table
- Periods/Series/Rows: horizontal rows on the periodic table.
- Groups/Families: vertical columns on the periodic table.
- Atomic mass/ radius: increases left/right and down.
- Valence electrons: electrons in the outermost energy level of an atom.
- Octet Rule: atoms tend to gain, lose, or share electrons to achieve a full set of eight valence electrons.
- Ions: atoms or groups of atoms with a net electric charge.
- Cations: positively charged ions.
- Anions: negatively charged ions.
- Electronegativity: a measure of an atom's ability to attract shared electrons. Higher electronegativity means greater attraction.
- Categories of elements: Alkali metals, Alkaline earth metals, Halogens, Noble gases.
Chemical Bonding
- Ionic bonds: bonds formed between a metal and a nonmetal.
- Polar covalent bonds: bonds formed between two nonmetals with unequal sharing of electrons.
- Nonpolar covalent bonds: bonds formed between two nonmetals with equal sharing of electrons.
- Metallic bonds: bonds in metals formed by a "sea of delocalized electrons."
- Polyatomic ions: ions containing more than one atom.
Physical vs. Chemical Changes
- Physical change: A change in state or form without changing the substance's composition (e.g., ice melting).
- Chemical change: A change in which a new substance or substances are formed, often irreversible, with changed composition (e.g., paper burning).
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Description
Test your knowledge about the types of bonds in chemistry, the properties of solutions, and the characteristics of different substances. This quiz will cover topics from covalent compounds to molarity calculations. Perfect for students studying chemistry concepts related to bonding and solubility.
