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Questions and Answers
What is the charge of a proton?
What is the charge of a proton?
The atomic number of an atom is the total number of protons and neutrons in its nucleus.
The atomic number of an atom is the total number of protons and neutrons in its nucleus.
False
What is the difference between an ionic bond and a covalent bond?
What is the difference between an ionic bond and a covalent bond?
An ionic bond is an electrostatic attraction between oppositely charged ions, while a covalent bond is the sharing of electrons between atoms.
The ____________ of an atom is the number of protons in its nucleus.
The ____________ of an atom is the number of protons in its nucleus.
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Match the following types of chemical reactions with their descriptions:
Match the following types of chemical reactions with their descriptions:
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The pH of a neutral solution is 0.
The pH of a neutral solution is 0.
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What is the trend of atomic radius across a period in the periodic table?
What is the trend of atomic radius across a period in the periodic table?
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What is the definition of an acid according to the Arrhenius theory?
What is the definition of an acid according to the Arrhenius theory?
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The pH of a solution is calculated using the formula pH = -log[___________].
The pH of a solution is calculated using the formula pH = -log[___________].
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What is the purpose of a catalyst in a chemical reaction?
What is the purpose of a catalyst in a chemical reaction?
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Study Notes
Atomic Structure
- Atomic model:
- Protons (positive charge) in the nucleus
- Neutrons (no charge) in the nucleus
- Electrons (negative charge) in energy levels (shells) around the nucleus
- Subatomic particles:
- Proton: +1 charge, 1 amu (atomic mass unit)
- Neutron: 0 charge, 1 amu
- Electron: -1 charge, negligible mass
- Atomic number (Z): number of protons in an atom's nucleus
- Mass number (A): total number of protons and neutrons in an atom's nucleus
Chemical Bonding
- Types of bonds:
- Ionic bond: electrostatic attraction between oppositely charged ions
- Covalent bond: sharing of electrons between atoms
- Bonding theories:
- Electronegativity: ability of an atom to attract electrons
- Electronegativity difference: predicts bond type (ionic or covalent)
Periodic Table
- Organization:
- Rows: periods (horizontal)
- Columns: groups (vertical)
- Periodic trends:
- Atomic radius decreases from left to right across a period
- Electronegativity increases from left to right across a period
- Blocks:
- s-block: first two columns (alkali metals and alkaline earth metals)
- p-block: last six columns (nonmetals and metalloids)
Chemical Reactions
- Types of reactions:
- Synthesis reaction: two substances combine to form a new compound
- Decomposition reaction: one substance breaks down into two or more substances
- Single displacement reaction: one element replaces another in a compound
- Combustion reaction: reaction with oxygen, often producing heat and light
- Reaction rates:
- Factors affecting rate: concentration, temperature, surface area, catalysts
Acids and Bases
- Arrhenius theory:
- Acid: substance that donates a proton (H+)
- Base: substance that accepts a proton
- pH scale:
- pH = -log[H+]
- Acidic: pH < 7
- Basic: pH > 7
- Neutral: pH = 7
Reactivity of Metals
- Reactivity series:
- Metals listed in order of reactivity (most reactive to least reactive)
- Reacts with oxygen, water, and acids to form compounds
- Extraction of metals:
- Methods: electrolysis, smelting, and refining
Writing the Formula
- Formula writing rules:
- Cations (positive ions) first
- Anions (negative ions) second
- Polyatomic ions: retain their charge and formula
- Formula types:
- Molecular formula: actual number of atoms in a molecule
- Empirical formula: simplest whole-number ratio of atoms in a molecule
Precipitation Reactions
- Definition: reaction resulting in the formation of an insoluble solid (precipitate)
- Conditions for precipitation:
- High concentration of reactants
- Presence of an electrolyte
- Net ionic equation: shows only the species participating in the reaction
Balancing the Equation
- Steps to balance an equation:
- Write the unbalanced equation
- Count the atoms of each element on both sides
- Add coefficients in front of formulas to balance the equation
- Balanced equation: number of atoms of each element is equal on both sides
Hydrocarbons
- Definition: compounds containing only carbon and hydrogen atoms
- Types of hydrocarbons:
- Saturated (single bonds only): alkanes
- Unsaturated (multiple bonds): alkenes and alkynes
- Functional groups:
- Alkyl group: hydrocarbon chain attached to a functional group
- Substituent: atom or group of atoms replacing a hydrogen atom
Atomic Structure
- Atomic model consists of protons, neutrons, and electrons
- Protons have a positive charge, neutrons have no charge, and electrons have a negative charge
- Electrons are arranged in energy levels (shells) around the nucleus
- Atomic number (Z) is the number of protons in an atom's nucleus
- Mass number (A) is the total number of protons and neutrons in an atom's nucleus
Chemical Bonding
- Ionic bonds form through electrostatic attraction between oppositely charged ions
- Covalent bonds form through the sharing of electrons between atoms
- Electronegativity is the ability of an atom to attract electrons
- Electronegativity difference predicts bond type (ionic or covalent)
Periodic Table
- The periodic table is organized into rows (periods) and columns (groups)
- Atomic radius decreases from left to right across a period
- Electronegativity increases from left to right across a period
- The s-block consists of the first two columns (alkali metals and alkaline earth metals)
- The p-block consists of the last six columns (nonmetals and metalloids)
Chemical Reactions
- Synthesis reactions involve two substances combining to form a new compound
- Decomposition reactions involve one substance breaking down into two or more substances
- Single displacement reactions involve one element replacing another in a compound
- Combustion reactions involve reaction with oxygen, often producing heat and light
- Factors affecting reaction rate include concentration, temperature, surface area, and catalysts
Acids and Bases
- Acids donate a proton (H+), while bases accept a proton
- pH is measured on a scale from 0 to 14, with 7 being neutral
- Acidic solutions have a pH < 7, basic solutions have a pH > 7
Reactivity of Metals
- The reactivity series lists metals in order of reactivity (most reactive to least reactive)
- Metals react with oxygen, water, and acids to form compounds
- Metals are extracted through electrolysis, smelting, and refining
Writing the Formula
- Cations are written first, followed by anions
- Polyatomic ions retain their charge and formula
- Molecular formula shows the actual number of atoms in a molecule
- Empirical formula shows the simplest whole-number ratio of atoms in a molecule
Precipitation Reactions
- Precipitation reactions result in the formation of an insoluble solid
- Conditions for precipitation include high concentration of reactants and presence of an electrolyte
- Net ionic equations show only the species participating in the reaction
Balancing the Equation
- The steps to balance an equation include writing the unbalanced equation, counting atoms, and adding coefficients
- A balanced equation has the same number of atoms of each element on both sides
Hydrocarbons
- Hydrocarbons are compounds containing only carbon and hydrogen atoms
- Saturated hydrocarbons (alkanes) have single bonds only
- Unsaturated hydrocarbons (alkenes and alkynes) have multiple bonds
- Alkyl groups are hydrocarbon chains attached to a functional group
- Substituents are atoms or groups of atoms replacing a hydrogen atom
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Description
Test your knowledge of atomic structure, including protons, neutrons, and electrons, as well as chemical bonding. Covers atomic number, mass number, and more.
