6. 3 Periodic Trends Summary: In general, atomic size increases from top to bottom within a group and decreases from left to right across.

 

10. 1 The Mole: A Measurement of Matter Summary: In general, there are three methods for measuring the amount of a substance. They are by count, by mass, and by volume. For example,.

 

5. 2 Electron arrangement in Atoms Summary: Three rules-the aufbau principle, the Pauli exclusion principle, and Hund’s rule – tell you how to find the electron.

 

1. 1 Chemistry Summary: Chemistry is the study of the composition and properties of matter and how they change. Matter is anything that has mass and occupies space. Since.

 

1. 3 Thinking Like a Scientist Summary: Alchemists are people who searched for a way to change cheap metals such as lead into gold. Practical alchemists.

 

5. 3 Physics and the Quantum Mechanical Model Summary: According to quantum mechanics, the motions of subatomic particles may be described as waves. The wavelength and frequency of light.

 

1. 4 Problem Solving in Chemistry Summary: Effective problem solving always involves developing a plan and then implementing that plan. Analyzing,.

 

5. 1 Models of Atom Summary: Rutherford’s planetary model states that in the nuclear atom, the protons and neutrons are located in the nucleus. The electrons are distributed.

 

11. 1 Describing Chemical Reactions Summary: A chemical reaction can be concisely represented by a chemical equation. The substances that undergo a chemical change are the reactants.

 

16. 1 Properties of Solutions Summary: Changes in the temperature of a system and the particle size of a solute alter the rate at which a solute dissolves. The extent to which.

 

14. 3 Ideal Gases Summary: The ideal gas law permits you to solve for the number of moles of a contained gas when the pressure, volume, and temperature are known. The ideal gas law is described.

 

Nuclear Transformations Summary: Nuclei that lie outside the band of stability undergo spontaneous radioactive decay. Nuclei with too many neutrons.

 

7. 3 Bonding in Metals Summary: Metals consist of closely packed cations that are surrounded by a sea of electrons. This arrangement constitutes the metallic bond.

 

13. 2 The Nature of Liquids Summary: Liquids are much denser than gases. Liquids and solids are known as condensed states of matter. The conversion of a liquid.

 

2. 1 Properties of Matter Summary: Properties used to describe matter can be classified as extensive or intensive. An extensive property is a property that depends on the amount.

 

22. 2 Unsaturated Hydrocarbons Summary: Alkenes are unsaturated hydrocarbons. That is, they contain one or more carbon-carbon double bonds. Alkynes are also unsaturated.

 

20. 1 The Meaning of Oxidation and Reduction Summary: or redox reactions are an important category of chemical reactions. Oxidation is losing electrons, and reduction is gaining electrons.

 

4. 1 Defining the atom Summary: An atom is the smallest particle of an element that retains its identify in a chemical reaction. Democritus was a Greek philosopher who was among.

 

7. 1 Ions Summary: Valence electrons are electrons in the highest occupied energy level of an element’s atoms. The number of valence electrons largely determines.

 

8. 2 The Nature of Covalent Bonding Summary: In covalent bonds, electron sharing usually occurs so that atoms attain the stable electron configurations.

 

10. 3 Percent Composition and Chemical Formulas Summary: To determine the percent by mass of any element in a given compound, divide the element’s mass by the mass of the compound.

 

4. 3 Distinguishing Among Atoms Summary: Elements are different because they have different numbers of protons. The atomic number of an element is the number.

 

22. 3 Isomers Summary: Isomers have the same molecular formula but different molecular. For example, 2-methylpropane is a structural isomer of butane. Isomers are different.

 

8. 4 Polar Bonds and Molecules Summary: When different atoms bond, the more electronegative atom attracts electrons more strongly and acquires.

 

3. 3 Conversion Problems Summary: A conversion factor is a ratio of equivalent measurements. Whenever two measurements are equal, or equivalent, a ratio of these two measurements will.

 

9. 4 Naming and Writing Formulas for Acids and Bases Summary: An acid is a combination of a monatomic or polyatomic anion with sufficient hydrogen atoms to make.

 

14. 2 The Gas Laws Summary: The pressure and volume of a fixed mass of gas are inversely related. If one decreases, the other increases. This relationship is known as Boyle’s law. As the pressure.

 

20. 2 Oxidation Number and Half of Reaction Summary: The oxidation number of an element in an uncombined state is zero. The oxidation number of a monatomic ion is the same e in magnitude.

 

16. 2 Concentrations of Solutions Summary: The relative amounts of solute and solvent in a solution can be described qualitatively as dilute or concentrated. Quantitative units of concentration include.

 

11. 2 Types of Chemical Reactions Summary: It is possible to predict the products of some chemical reactions. In order to do this, you must be able to recognize at least.

 

11. 3 Reactions in Aqueous Solution Summary: Many important chemical reactions take place in water, which makes up 66 percent of human body.

 

3. 1 Measurements and their Uncertainty Summary: Measurements are fundamental to the experimental sciences. A measurement is a quantity that has both a number and a unit. It is important to be ale to make.

 

10. 2 Mole-Mass and Mole-Volume Relationships Summary: The molar mass of an element or compound is the conversion factor for converting between the mass and the number of moles of a substance.

 

2. 4 Chemical Reaction Summary: The ability of a substance to undergo a specific chemical change is called a chemical property. For example, the ability of rust is a chemical.

 

13. 1 The Nature of Gases Summary: Particles in a gas are considered to be small, hard spheres with an insignificant volume. The motion of the particles in a gas is rapid, constant, and random.

 

17. 1 The Flow of Energy-Heat and Work Summary: The energy that flows from a warm object to a cool object is called heat. The energy stored.

 

9. 2 Naming and Writing Formulas for Ionic Compounds Summary: The name of a binary ionic compound is the cation name followed by the anion name. Names.

 

9. 3 Naming and Writing Formulas for Molecular Compounds Summary: Binary molecular compounds are composed of two nonmetallic elements. They are composed of molecules. For example,.

 

4. 2 Structure of the Nuclear Atom Summary: Three types of subatomic particles are electrons, protons, and neutrons. Electrons are negatively charged subatomic particles,.

 

14. 1 Properties of Gases Summary: Gas are easily compressed or squeezed into a smaller volume because of the space between particles in a gas. The four variables used.

 

3. 2 The International System of Units SI Summary: Five commonly used SI base units are the meter, kilogram, kelvin, second, and mole. Common metric.

 

7. 2 ionic Bonds and Ionic Compounds Summary: Ionic compounds are produced by the attraction between cations and anions by electrostatic forces. The forces that.

 

6. 2 Classifying the Elements Summary: The periodic table displays the chemical symbols and names of the elements. It also provides the information about the structure of their.

 

9. 1 Naming Ions Summary: Ions that consist of a single atom are called monatomic ions. Metallic elements tend to lose electrons.

 

25. 1 Nuclear Radiation Summary: Isotopes with unstable nuclei are radioactive and are called radioisotopes. The nuclei of radioisotopes decay to stable nuclei plus.

 

25. 3 Fission and fusion of atomic nuclei Summary: Nuclear fission occurs when fissionable isotopes are bombarded with neutrons. The fissionable atom.

 

19. 1 Acid-Base Theories Summary: Compounds can be classified as acids or bases according to three different theories. An Arrhenius acid yields hydrogen ions.

 

14. 4 Gases: Mixtures and Movements Summary: According to Dalton’s law of partial pressures, at constant volume and temperature, the total pressure exerted by a mixture of gases.

 

13. 4 Changes of State Summary: The change that occurs when a solid goes directly to the gas or vapor state without first becoming a liquid.