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Questions and Answers
What is the primary difference between ionic and molecular compounds?
What is the naming convention for ionic compounds?
What is the mole concept used to express?
What is the relationship between pressure and volume according to Boyle's Law?
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What is the pH of a neutral solution?
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What is the characteristic of a strong acid?
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What is the function of a base in a chemical reaction?
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What is the formula for the ideal gas law?
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What is the primary focus of biochemistry?
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Which subdiscipline of physical chemistry involves the study of the relationships between heat, work, and energy?
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What is the typical characteristic of ionic compounds?
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How many particles are represented by one mole?
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What is the purpose of the mole concept in chemistry?
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Which of the following is an example of a molecular compound?
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What is the focus of enzymology?
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What is the study of the rates of chemical reactions?
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What is the unit of the gas constant R in the ideal gas law?
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What is the function of an acid in a chemical reaction?
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What is the relationship between the volume and temperature of a gas at constant pressure?
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What is the result of a polar covalent bond?
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How can the dipole moment of a bond be calculated?
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What is the unit of molar mass?
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Study Notes
Ionic Compounds
- Formed from the attraction between oppositely charged ions (cation and anion)
- Typically composed of a metal and a nonmetal
- Examples: NaCl (sodium chloride), CaCO3 (calcium carbonate)
- Naming conventions:
- Cation first, then anion
- Use roman numerals to indicate charge of cation (if necessary)
- Use -ide suffix for anion
Molecular Compounds
- Formed from the sharing of electrons between nonmetal atoms
- Typically composed of two or more nonmetals
- Examples: H2O (water), CO2 (carbon dioxide)
- Naming conventions:
- Use prefixes to indicate number of atoms (mono-, di-, tri-, etc.)
- Use the full name of the first element, then the full name of the second element with an -ide suffix
The Mole Concept
- A mole (mol) is a unit of measurement, defined as 6.022 x 10^23 particles
- Used to express the amount of a substance
- Molar mass: the mass of one mole of a substance, in grams
- Calculating moles: moles = mass / molar mass
Gas Laws
- Boyle's Law: P1V1 = P2V2 (pressure and volume are inversely proportional)
- Charles' Law: V1/T1 = V2/T2 (volume and temperature are directly proportional)
- Avogadro's Law: V = nRT (volume is proportional to number of moles and temperature)
- Ideal Gas Law: PV = nRT (combines the above laws)
- Gay-Lussac's Law: P1/T1 = P2/T2 (pressure and temperature are directly proportional)
Acidity and Basicity
- pH: a measure of the concentration of hydrogen ions (H+), ranging from 0-14
- pOH: a measure of the concentration of hydroxide ions (OH-), ranging from 0-14
-
Acids:
- Donors of H+ ions
- Examples: HCl (hydrochloric acid), H2SO4 (sulfuric acid)
-
Bases:
- Acceptors of H+ ions
- Examples: NaOH (sodium hydroxide), Ca(OH)2 (calcium hydroxide)
- Strong Acids: completely dissociate in water, releasing all H+ ions
- Weak Acids: partially dissociate in water, releasing some H+ ions
- Strong Bases: completely dissociate in water, releasing all OH- ions
- Weak Bases: partially dissociate in water, releasing some OH- ions
Ionic Compounds
- Attraction between oppositely charged ions (cation and anion) forms ionic compounds
- Typically composed of a metal and a nonmetal
- Examples: sodium chloride (NaCl), calcium carbonate (CaCO3)
- Cation always comes first in the naming convention, followed by the anion
- Roman numerals are used to indicate the charge of the cation if necessary
- -ide suffix is used for the anion
Molecular Compounds
- Formed from the sharing of electrons between nonmetal atoms
- Typically composed of two or more nonmetals
- Examples: water (H2O), carbon dioxide (CO2)
- Prefixes are used to indicate the number of atoms in the molecular compound (mono-, di-, tri-, etc.)
- Full name of the first element is followed by the full name of the second element with an -ide suffix
The Mole Concept
- One mole (mol) is equal to 6.022 x 10^23 particles
- Mole is used to express the amount of a substance
- Molar mass is the mass of one mole of a substance, expressed in grams
- Moles can be calculated by dividing the mass by the molar mass
Gas Laws
- Boyle's Law states that pressure and volume are inversely proportional
- Charles' Law states that volume and temperature are directly proportional
- Avogadro's Law states that volume is proportional to the number of moles and temperature
- Ideal Gas Law combines the previous laws, stating that PV = nRT
- Gay-Lussac's Law states that pressure and temperature are directly proportional
Acidity and Basicity
- pH is a measure of the concentration of hydrogen ions (H+), ranging from 0-14
- pOH is a measure of the concentration of hydroxide ions (OH-), ranging from 0-14
- Acids are donors of H+ ions, examples include hydrochloric acid (HCl) and sulfuric acid (H2SO4)
- Bases are acceptors of H+ ions, examples include sodium hydroxide (NaOH) and calcium hydroxide (Ca(OH)2)
- Strong acids completely dissociate in water, releasing all H+ ions
- Weak acids partially dissociate in water, releasing some H+ ions
- Strong bases completely dissociate in water, releasing all OH- ions
- Weak bases partially dissociate in water, releasing some OH- ions
Biochemistry
- Biochemistry is the study of the chemical processes that occur within living organisms
- Involves the structure and function of biomolecules such as carbohydrates, proteins, and nucleic acids
- Subdisciplines include structural biology, enzymology, and metabolism
Physical Chemistry
- Physical chemistry is the study of the physical principles underlying chemical reactions and processes
- Involves the application of physical laws and concepts to understand chemical phenomena
- Subdisciplines include thermodynamics, kinetics, and spectroscopy
Ionic and Molecular Compounds
- Ionic compounds are formed by the transfer of electrons between atoms
- Characteristics of ionic compounds:
- High melting and boiling points
- Examples: NaCl (table salt), CaCO3 (calcium carbonate)
- Molecular compounds are formed by the sharing of electrons between atoms
- Characteristics of molecular compounds:
- Lower melting and boiling points
- Examples: H2O (water), CO2 (carbon dioxide)
The Mole Concept
- A mole (mol) is a unit of measurement that represents 6.022 x 10^23 particles
- Used to express the amount of a substance in a chemical reaction
- Steps in mole calculations:
- Identify the number of moles of reactants
- Use the balanced equation to determine the number of moles of products
- Convert between moles and grams using the molar mass
Gas Laws
- Ideal Gas Law: PV = nRT
- Relates the pressure, volume, and temperature of an ideal gas
- R is the gas constant
- Charles' Law: V1 / T1 = V2 / T2
- Relates the volume and temperature of a gas at constant pressure
- Boyle's Law: P1V1 = P2V2
- Relates the pressure and volume of a gas at constant temperature
- Avogadro's Law: V = nRT / P
- Relates the volume and number of moles of a gas at constant temperature and pressure
Acidity and Basicity
- Acids are donors of H+ ions (protons)
- Examples: HCl (hydrochloric acid), H2SO4 (sulfuric acid)
- Bases are acceptors of H+ ions
- Examples: NaOH (sodium hydroxide), KOH (potassium hydroxide)
- pH Scale: measures the concentration of H+ ions in a solution
- pH < 7: acidic
- pH > 7: basic
- pH = 7: neutral
Bond Polarity
- Polar covalent bonds are formed when two atoms share electrons unequally
- Results in a partial positive charge (δ+) on one atom and a partial negative charge (δ-) on the other
- Electronegativity: the ability of an atom to attract electrons in a covalent bond
- Dipole moment: a measure of the polarity of a bond or molecule
- Calculated using the formula: μ = δ x d
- Where μ is the dipole moment, δ is the partial charge, and d is the distance between the atoms
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Description
Learn about the formation and naming conventions of ionic compounds, composed of metals and nonmetals, and molecular compounds formed from nonmetal atoms.
