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Questions and Answers
Which of the following subatomic particles has a negative charge?
What is the maximum number of electrons that can be held in the first electron shell?
Which type of chemical bond is formed by the transfer of electrons between atoms?
What is the mass of a proton in atomic mass units (amu)?
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Which of the following electron configurations is an example of a correct notation?
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What is the primary characteristic of a hydrogen bond?
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Which of the following states of matter has a fixed shape and volume?
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What is the process of changing from a liquid to a gas?
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What is the unit of measurement that represents 6.022 x 10^23 particles?
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What is the formula that represents the simplest whole-number ratio of atoms in a compound?
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Study Notes
Atomic Structure
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Atomic Model: The modern atomic model consists of:
- Protons (positive charge) in the nucleus
- Neutrons (no charge) in the nucleus
- Electrons (negative charge) in energy levels around the nucleus
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Electron Configuration:
- Electron shells (energy levels) have a maximum number of electrons
- The first shell can hold up to 2 electrons, the second shell up to 8, and so on
- Electron configuration notation: 1s2 2s2 2p6 (example)
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Subatomic Particles:
- Protons: positively charged, mass of 1 amu (atomic mass unit)
- Neutrons: no charge, mass of 1 amu
- Electrons: negatively charged, negligible mass
Chemical Bonding
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Types of Chemical Bonds:
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Ionic Bonds: Formed by the transfer of electrons between atoms
- Cations (positively charged) and anions (negatively charged) attract each other
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Covalent Bonds: Formed by the sharing of electrons between atoms
- Polar covalent bonds: unequal sharing of electrons, resulting in a partial charge
- Nonpolar covalent bonds: equal sharing of electrons
- Hydrogen Bonds: Weak bonds between hydrogen and highly electronegative atoms (F, O, N)
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Ionic Bonds: Formed by the transfer of electrons between atoms
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Bond Properties:
- Bond length: distance between the nuclei of two bonded atoms
- Bond energy: energy required to break a bond
- Bond polarity: difference in electronegativity between bonded atoms
States of Matter
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Solid:
- Particles are closely packed and vibrate in place
- Has a fixed shape and volume
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Liquid:
- Particles are close together but able to move past each other
- Has a fixed volume but takes the shape of its container
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Gas:
- Particles are widely spaced and move freely
- Has neither a fixed shape nor volume
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Phase Changes:
- Melting: solid to liquid
- Freezing: liquid to solid
- Vaporization: liquid to gas
- Condensation: gas to liquid
Stoichiometry
- Mole: A unit of measurement, 6.022 x 10^23 particles (atoms, molecules, ions)
- Molar Mass: The mass of one mole of a substance, in grams
- Empirical Formula: The simplest whole-number ratio of atoms in a compound
- Molecular Formula: The actual number of atoms in a molecule
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Stoichiometric Calculations:
- Moles of reactants to moles of products
- Mass of reactants to mass of products
- Limiting reagent: the reactant that determines the amount of product formed
Atomic Structure
- Atomic model consists of protons, neutrons, and electrons
- Protons have a positive charge and neutrons have no charge, both are found in the nucleus
- Electrons have a negative charge and are found in energy levels around the nucleus
- Electron shells have a maximum number of electrons, with the first shell holding up to 2 electrons, the second shell up to 8, and so on
- Electron configuration notation is used to describe the arrangement of electrons in an atom, for example, 1s2 2s2 2p6
Subatomic Particles
- Protons have a mass of 1 amu (atomic mass unit) and a positive charge
- Neutrons have a mass of 1 amu and no charge
- Electrons have a negligible mass and a negative charge
Chemical Bonding
- Chemical bonds are formed between atoms through the transfer or sharing of electrons
- Ionic bonds are formed by the transfer of electrons, resulting in positively charged cations and negatively charged anions that attract each other
- Covalent bonds are formed by the sharing of electrons between atoms, resulting in a molecule
- Polar covalent bonds involve unequal sharing of electrons, resulting in a partial charge, while nonpolar covalent bonds involve equal sharing of electrons
- Hydrogen bonds are weak bonds between hydrogen and highly electronegative atoms such as fluorine, oxygen, and nitrogen
Bond Properties
- Bond length is the distance between the nuclei of two bonded atoms
- Bond energy is the energy required to break a bond
- Bond polarity is the difference in electronegativity between bonded atoms
States of Matter
- In a solid, particles are closely packed and vibrate in place, having a fixed shape and volume
- In a liquid, particles are close together but able to move past each other, having a fixed volume but taking the shape of its container
- In a gas, particles are widely spaced and move freely, having neither a fixed shape nor volume
- Phase changes occur when a substance changes from one state of matter to another, such as melting, freezing, vaporization, and condensation
Stoichiometry
- A mole is a unit of measurement, equal to 6.022 x 10^23 particles (atoms, molecules, or ions)
- Molar mass is the mass of one mole of a substance, in grams
- The empirical formula is the simplest whole-number ratio of atoms in a compound
- The molecular formula is the actual number of atoms in a molecule
- Stoichiometric calculations involve the mole ratio of reactants to products, and the mass ratio of reactants to products
- The limiting reagent is the reactant that determines the amount of product formed
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Description
Learn about the modern atomic model, electron configuration, and subatomic particles. Test your knowledge of protons, neutrons, electrons, and energy levels.