Chem unit 2 presentation
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This document provides an overview of chemistry unit 2 which covers how matter changes. It discusses the three common states of matter - solids, liquids and gases. It defines physical and chemical properties and changes. It also defines mixtures and how they are combinations of substances that can be separated. It introduces elements and compounds, explaining how compounds are combinations of elements that have different properties. It covers the laws of definite and multiple proportions for compounds.
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Chem unit 12 presentation
Here is a one page paper relating chemistry and gases:
Chemistry and gases are intimately related. Many of the most important discoveries and applications in chemistry involve gases. Historically, scientists like Robert Boyle, Jacques Charles, and Joseph Gay-Lussac made seminal discoveries about gas behavior through careful experimentation. Their gas laws laid the foundation for understanding the properties and interactions of gases.
One area where gases play a huge role is in industry and energy. The Haber process converts nitrogen gas and hydrogen gas into ammonia, a key component of fertilizers that have enabled the growth of the global population. Natural gas, composed primarily of methane, heats homes and fuels power plants around the world. Greenhouse gases like carbon dioxide
Ap chem unit 15 presentation
Here are the ratios [HA]/[A-] required for each system to yield a pH of 4.30:
Acetic acid (pKa = 4.76): [HA]/[A-] = 1
Benzoic acid (pKa = 4.19): [HA]/[A-] = 1
Phthalic acid (pKa = 2.89): [HA]/[A-] is not possible since the pKa is too low.
The optimal system is acetic acid/sodium acetate since it has a pKa closest to the desired pH of 4.30. This system allows a ratio of [HA]/[A-] = 1, which provides maximum buffering
Chem 1 unit 11 presentation
* Given: 0.85 g of gas dissolves in 1 L of water at 4 atm
* Let's call the amount that will dissolve at 1 atm = S1
* Using Henry's Law: S1/S2 = P1/P2
* S2 is the amount we want to find at 1 atm
* P1 = 4 atm
* P2 = 1 atm
* S1 = 0.85 g
* Substitute into Henry's Law equation:
* 0.85/S2 = 4/1
* S2 = 0.85 * 1/4 = 0.2125 g
Therefore, the amount that will dissolve in 1 L of water at 1 atm is
Chem 1 unit 11 presentation
Solutions can be either homogeneous or heterogeneous mixtures. Concentration of solutions can be expressed in terms of percent, moles, molarity, or molality. Factors such as temperature, pressure, and polarity affect the solubility and formation of solutions. Colligative properties depend on the number of solute particles in solution. Stoichiometry can be used to solve solution reaction problems by considering the concentrations of reactants and products.
Chem 1 unit 11 presentation
Solutions can be either homogeneous, made of one phase, or heterogeneous, made of two or more distinct phases. Concentration of a solution can be expressed in terms of percent composition, molarity, or molality. Factors such as temperature, pressure, and polarity affect the solubility and formation of solutions. Stoichiometry can be used to solve problems involving the concentrations of reactants and products in solution.
Chem 1 unit 11 presentation
Solutions can be either homogeneous, made of one phase, or heterogeneous, made of two or more distinct phases. Concentration of a solution can be expressed in terms of percent composition, molarity, or molality. Factors such as temperature, pressure, and polarity affect the solubility and formation of solutions. Stoichiometry can be used to solve problems involving reactions in solution by using molar concentrations.
Ap chem unit 14 presentation part 2
This document discusses several key topics regarding bases:
1. The hydroxides of Group 1 and 2 elements are strong bases, with NaOH and KOH being common laboratory reagents. The alkaline earth hydroxides have low solubility.
2. Calculating the pH of a solution involves determining the hydroxide ion concentration from any reacting species. A 5.0x10-2 M NaOH solution has a pH of 12.70.
3. Many bases other than hydroxides can produce hydroxide ions through reaction with water, such as ammonia. Calculations for weak bases are similar to weak acids.
4. Salts can behave as acids or bases depending on
Ap chem unit 14 presentation part 2
The document discusses several key topics regarding acids and bases:
1. Group 1 and 2 hydroxides such as LiOH, NaOH, and Ca(OH)2 are strong bases. NaOH and KOH are common laboratory reagents while alkaline earth hydroxides have low solubility.
2. Calculating pH involves determining the hydroxide ion concentration from solubility equations or acid/base equilibria. Examples show calculating the pH of NaOH and NH3 solutions.
3. Many bases like NH3 produce hydroxide ions when dissolved in water by reacting with water. The acid dissociation constant Kb describes this reaction.
4. Polyprotic acids dissociate
Ap chem unit 14 presentation part 1
[H+] = 2.7x10-2 M
pH = 1.57
The calculated [H+] is within ±5% of Ka, so the
approximation is valid. The pH is 1.57.
Chem unit 10 presentation
Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions based on mole ratios from balanced equations. Key concepts include:
1) Balanced equations show mole, mass, and particle relationships between reactants and products
2) Limiting reactants determine the maximum amount of product that can be formed
3) Excess reactants remain after the limiting reactant is used up in the reaction
Chem unit 8 presentation
Polyatomic ions stay intact in aqueous solutions because they are held together by strong covalent bonds between their constituent atoms. When ionic compounds dissolve in water, the ions separate but polyatomic ions remain intact units because the covalent bonds within them are not broken by the dissociation process.
Chemistry unit 9 presentation
The correct formula for an ionic compound must contain positive and negative ions in a ratio to achieve an overall neutral charge. CO2 is a molecular compound and does not contain ions, so the answer is A.
Ap chem unit 13 presentation
This document discusses chemical equilibrium, including:
- Reactions reach equilibrium when concentrations of reactants and products remain constant over time.
- The equilibrium constant, K, quantifies the position of equilibrium and can be used to calculate concentrations at equilibrium.
- Equilibrium expressions can involve gas concentrations or pressures, and heterogeneous equilibria only include gases and dissolved substances in expressions.
- Knowing K allows prediction of whether a reaction will occur and the direction a system will shift to reach equilibrium.
Chem unit 8 presentation
This document discusses chemical reactions and how they are represented. It covers the following key points:
1. Chemical reactions are represented by balanced chemical equations that show the reactants and products. There are four main types of reactions: synthesis, combustion, decomposition, and replacement.
2. Double replacement reactions occur between ionic compounds in aqueous solution and often produce a precipitate, water, or a gas.
3. Chemical equations must be balanced to obey the law of conservation of mass. This involves determining coefficients for the reactants and products so that the number of atoms of each element is equal on both sides of the reaction.
Ap chem unit 12 presentation
The half-life of N2O5 for a first order reaction is:
t1/2 = ln(2)/k
= ln(2)/(6.93 x 10-3 s-1)
= 100 s
So every 100 seconds, the concentration of N2O5 will be half of what it was 100 seconds earlier.
Chem unit 7 presentation
Here are the key points about polar and nonpolar covalent bonds:
- Nonpolar covalent bonds form between atoms with similar electronegativity. Electrons are shared equally. Examples include H2, Cl2, etc.
- Polar covalent bonds form between atoms with different electronegativity. Electrons are pulled slightly closer to the more electronegative atom. This creates partial positive and negative charges called dipoles.
- Molecules with polar bonds are polar molecules. They are attracted to electric fields due to the separation of charge in the dipoles. Water is a common example.
- Molecules with nonpolar covalent bonds have equal charge distribution and are nonpolar molecules. They
Chem unit 6 presentation
Ionic bonds form when oppositely charged ions attract each other, forming ionic compounds. Cations form when atoms lose electrons to achieve a stable electron configuration, while anions form when atoms gain electrons. Ionic compounds consist of a crystal lattice structure where cations are surrounded by anions. They have properties like high melting points and boiling points since energy is required to overcome the strong electrostatic attractions between ions.
Ap chem unit 11 presentation
This document discusses several topics related to solutions, including:
1. It defines solutions and describes ways to express concentration such as molarity, mass percent, and mole fraction.
2. It explains that the enthalpy of solution depends on the energies required to separate the solute, expand the solvent, and allow interactions between solute and solvent particles. The overall enthalpy can be endothermic or exothermic.
3. Factors that affect solubility include like dissolving like, pressure, temperature, and molecular structure. Henry's law relates the solubility of gases to pressure. Temperature can either increase or decrease solubility depending on the substances involved.
Chem unit 7 presentation
Here are the key points about polar and nonpolar covalent bonds:
- Nonpolar covalent bonds form between atoms with similar electronegativity. Electrons are equally shared. Examples include H2, Cl2, etc.
- Polar covalent bonds form between atoms with different electronegativity. Electrons are unequally shared, resulting in partial positive and negative charges on the atoms. Examples include HCl, H2O.
- Polar molecules are attracted to each other due to their partial charges. They are soluble in polar solvents like water. Nonpolar molecules are not attracted and are soluble in nonpolar solvents like hexane.
- Most bonds have some ionic character based on electrone
Chem unit 6 presentation
Ionic compounds form when oppositely charged ions attract each other, forming ionic bonds. Ions are formed when atoms gain or lose valence electrons to achieve a stable electron configuration. In ionic compounds, the cation is written first followed by the anion in chemical formulas. Metals form metallic bonds where metal atoms donate their valence electrons, which are free to move throughout the crystal lattice structure.
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Chem unit 2 presentation
- 1. Chemistry Unit 2 How does matter change?
- 2. How does matter change?
- 7. Physical Properties of Matter A physical property is a characteristic that can be observed or measured without changing the sample ’s composition.
- 14. Chemical Changes A change that involves one or more substances turning into new substances is called a chemical change . Examples: Decomposing, rusting, exploding, burning, or oxidizing are all terms that describe chemical changes.
- 20. Mixtures
- 29. Compounds
- 31. Percent by Mass The relative amounts are expressed as percent by mass , the ratio of the mass of each element to the total mass of the compound expressed as a percentage.
- 40. How does matter change?
- 45. The End