Solutions!
... Factors Affecting How Fast Particles Dissolve 1.) Stirring makes compounds dissolve faster. ...
... Factors Affecting How Fast Particles Dissolve 1.) Stirring makes compounds dissolve faster. ...
Chemistry - Chap 12 Homework Answers 2014
... b. C4H10 (l) or C8H18(l) both have only disp but octane is much larger. same reason as above c. HCl (l) or H2O (l) HCl has disp and dipole but water has all 3. same reasons. d.. Br2 or PH3 bromine has disp whiles PH3 is disp, and dipole so same reason e. H2O or NH3 both have disp, and H bonding. Wat ...
... b. C4H10 (l) or C8H18(l) both have only disp but octane is much larger. same reason as above c. HCl (l) or H2O (l) HCl has disp and dipole but water has all 3. same reasons. d.. Br2 or PH3 bromine has disp whiles PH3 is disp, and dipole so same reason e. H2O or NH3 both have disp, and H bonding. Wat ...
Ionic Equations
... • Solutions of non-electrolytes have very low conductivities, since they produce no ions – Most molecular substances are non-electrolytes – Exceptions are acidic and basic molecules such as HCl(g) and NH3(g) ...
... • Solutions of non-electrolytes have very low conductivities, since they produce no ions – Most molecular substances are non-electrolytes – Exceptions are acidic and basic molecules such as HCl(g) and NH3(g) ...
Decomposition Reaction
... very active metals and they react with cold water to produce the hydroxide and hydrogen gas. 3. The next four metals (magnesium - chromium) are considered active metals and they will react with very hot water or steam to form the oxide and hydrogen gas. 4. The oxides of all of these first metals res ...
... very active metals and they react with cold water to produce the hydroxide and hydrogen gas. 3. The next four metals (magnesium - chromium) are considered active metals and they will react with very hot water or steam to form the oxide and hydrogen gas. 4. The oxides of all of these first metals res ...
Vocabulary Notes
... A bond formed through the transfer of electrons. They are held by electrostatic forces. ...
... A bond formed through the transfer of electrons. They are held by electrostatic forces. ...
FALL Final Review KEY
... 37. If the difference in electronegativity is greater than 1.7, then it is ionic bonding If the difference in electronegativity is less than 1.7, then it is covalent bonding (less than 0.5 is nonpolar covalent and between 0.5-1.6 is polar covalent) 38. NaCl: ionic, NaOH: ionic and covalent, BaSO4: i ...
... 37. If the difference in electronegativity is greater than 1.7, then it is ionic bonding If the difference in electronegativity is less than 1.7, then it is covalent bonding (less than 0.5 is nonpolar covalent and between 0.5-1.6 is polar covalent) 38. NaCl: ionic, NaOH: ionic and covalent, BaSO4: i ...
s - chem116
... To write a net ionic equation from the newly created ionic equation: Na+ + Cl- + Ag+ + NO3- Na+ + NO3- + AgCl Simply eliminate any ion that appears on both the reactant and product side of the equation (shown in orange). ...
... To write a net ionic equation from the newly created ionic equation: Na+ + Cl- + Ag+ + NO3- Na+ + NO3- + AgCl Simply eliminate any ion that appears on both the reactant and product side of the equation (shown in orange). ...
Study Sheet
... Know the two big driving forces of the universe: tend toward minimum Enthalpy (H) … potential energy tend toward maximum Entropy (S) … randomness… disorder… (Note: Our book does not cover entropy until chapter 18) ...
... Know the two big driving forces of the universe: tend toward minimum Enthalpy (H) … potential energy tend toward maximum Entropy (S) … randomness… disorder… (Note: Our book does not cover entropy until chapter 18) ...
8.1 Classifying inorganic compounds
... Inorganic molecular compounds are molecules formed with 2 non-metals (but no C or very little C!). ...
... Inorganic molecular compounds are molecules formed with 2 non-metals (but no C or very little C!). ...
Document
... that accounts for the apparent decrease of concentration because of interaction with other ions in solution. The value of γ can be estimated using one of the existing activity models. Finding appropriate activity coefficients for aqueous species especially in concentrated multicomponent solutions is ...
... that accounts for the apparent decrease of concentration because of interaction with other ions in solution. The value of γ can be estimated using one of the existing activity models. Finding appropriate activity coefficients for aqueous species especially in concentrated multicomponent solutions is ...
1 - mvhs-fuhsd.org
... 12. Is each of the properties below a physical or chemical property? a. Temperature at which a solid is converted to a liquid b. Odor c. Temperature at which a compound breaks down into its elements d. Oxygen reacts with a substance to produce energy 13. Which of the substances below are mixtures, a ...
... 12. Is each of the properties below a physical or chemical property? a. Temperature at which a solid is converted to a liquid b. Odor c. Temperature at which a compound breaks down into its elements d. Oxygen reacts with a substance to produce energy 13. Which of the substances below are mixtures, a ...
Bonding Notes
... Ionic bonds can happen when metals and non-metals (especially halogens, Oxygen, or Sulfur) react: 2Na(s) + Cl2(g) —> 2NaCl(s) [the subscripts (s) and (g) indicate solid and gas states respectively] They also can form when the ions already exist, such as when a solution evaporates: [the subscript (aq ...
... Ionic bonds can happen when metals and non-metals (especially halogens, Oxygen, or Sulfur) react: 2Na(s) + Cl2(g) —> 2NaCl(s) [the subscripts (s) and (g) indicate solid and gas states respectively] They also can form when the ions already exist, such as when a solution evaporates: [the subscript (aq ...
Chapter 13 notes
... Properties of Electrolyte Solutions Conductivity of Solutions To compare the conductivities of strong and weak electrolytes, the conductivities of solutions of equal concentration must be compared. Ionization of pure water: H2O(l) + H2O(l) So why does water that comes out of the tap conduct electric ...
... Properties of Electrolyte Solutions Conductivity of Solutions To compare the conductivities of strong and weak electrolytes, the conductivities of solutions of equal concentration must be compared. Ionization of pure water: H2O(l) + H2O(l) So why does water that comes out of the tap conduct electric ...
PS_CHEM7_ch4 - WordPress.com
... • d) Ethylene glycol (HOCH2CH2OH) molecules contain polar O–H bonds, similar to water, so it would be expected to be soluble. ...
... • d) Ethylene glycol (HOCH2CH2OH) molecules contain polar O–H bonds, similar to water, so it would be expected to be soluble. ...
Unit 2 Assignments Answers
... (a) 0.0618 m or 0.618 mol/kg (b) 2.03 m or 2.03 mol/kg (a) 1.74 m or 1.74 mol/kg (b) 0.87 m or 0.87 mol/kg (c) 6.99 m or 6.99 mol/kg 3.0 × 102 g or 0.30 kg 17.3 M or 17.3 mol/L Most ionic compounds (because they are solids in room temperature) usually have increase solubility in water as temperature ...
... (a) 0.0618 m or 0.618 mol/kg (b) 2.03 m or 2.03 mol/kg (a) 1.74 m or 1.74 mol/kg (b) 0.87 m or 0.87 mol/kg (c) 6.99 m or 6.99 mol/kg 3.0 × 102 g or 0.30 kg 17.3 M or 17.3 mol/L Most ionic compounds (because they are solids in room temperature) usually have increase solubility in water as temperature ...
Chemistry 111: Exam 1 Topics
... Recognize that you have to solve this type of problem – should have 4 out of 5 gas variables. Set up a table to solve the problem! Be able to use equation for gas density. Use n=PV/RT for stoichoimetry (ugh) Sometimes cheat - @ STP have 22.4 L/mol of any gas ...
... Recognize that you have to solve this type of problem – should have 4 out of 5 gas variables. Set up a table to solve the problem! Be able to use equation for gas density. Use n=PV/RT for stoichoimetry (ugh) Sometimes cheat - @ STP have 22.4 L/mol of any gas ...
Chapter 6.2 Notes
... - because they do not form individual molecules, to write the chemical formulas use the smallest ratio of one ion to another, called the formula unit NaCl 1:1 Na2O 2:1 AlBr3 1:3 - smallest ratio means they will not be divisible by each other and get a whole number - will never have an ionic compound ...
... - because they do not form individual molecules, to write the chemical formulas use the smallest ratio of one ion to another, called the formula unit NaCl 1:1 Na2O 2:1 AlBr3 1:3 - smallest ratio means they will not be divisible by each other and get a whole number - will never have an ionic compound ...
Objectives
... MAIN IDEA: Atoms bond with each other by transferring or sharing valence electrons to form compounds. ...
... MAIN IDEA: Atoms bond with each other by transferring or sharing valence electrons to form compounds. ...
FORMULA WRITNG
... 2) Write the synthesis of each of the following compounds from their elements. a. sodium bromide b. potassium nitride c. sodium carbonate ...
... 2) Write the synthesis of each of the following compounds from their elements. a. sodium bromide b. potassium nitride c. sodium carbonate ...
States of Matter
... Molar mass can be used for m, and the effusion rate is directly proportional to v Example problem: Find the molar mass of a gas that effuses at a rate twice as slow as helium. ...
... Molar mass can be used for m, and the effusion rate is directly proportional to v Example problem: Find the molar mass of a gas that effuses at a rate twice as slow as helium. ...
Lecture 3: Solubility of Gases, Liquids, and Solids in Liquids ΔG
... The complicating issue is the heat of mixing-- ∆H can be either endo or exothermic and is quite varied ∆Hsoln is (+) for NaCl in H2O ∆Hsoln is (–) for Na2SO4 in H2O ∆Hsoln is (–) for O2 in H2O Consider the case that ∆Hmix is negative: since ∆Smix is positive then ∆Gsoln will have to be negative and ...
... The complicating issue is the heat of mixing-- ∆H can be either endo or exothermic and is quite varied ∆Hsoln is (+) for NaCl in H2O ∆Hsoln is (–) for Na2SO4 in H2O ∆Hsoln is (–) for O2 in H2O Consider the case that ∆Hmix is negative: since ∆Smix is positive then ∆Gsoln will have to be negative and ...
CHEMISTRY 211, Lect. Sect. 003
... Calculate ∆G° for the reaction below and tell whether it is spontaneous or nonspontaneous under standard conditions at 25°C. 2S(s) + 3O2 (g) + 2H2O(l) → 2H2SO4(l) ; ∆H° = -1056 kJ/mol; ∆S°= -505 J/mol (a) (b) (c) (d) ...
... Calculate ∆G° for the reaction below and tell whether it is spontaneous or nonspontaneous under standard conditions at 25°C. 2S(s) + 3O2 (g) + 2H2O(l) → 2H2SO4(l) ; ∆H° = -1056 kJ/mol; ∆S°= -505 J/mol (a) (b) (c) (d) ...
Molecules and Ions
... Molecules and their Chemical Formulas There are two ways of describing the components (i.e. the number and type of atoms) found inside any molecule: Molecular Formula: the actual number and type of atoms in a compound, e.g. hydrogen peroxide = H2O2 Empirical Formula: the lowest whole number ratio of ...
... Molecules and their Chemical Formulas There are two ways of describing the components (i.e. the number and type of atoms) found inside any molecule: Molecular Formula: the actual number and type of atoms in a compound, e.g. hydrogen peroxide = H2O2 Empirical Formula: the lowest whole number ratio of ...
Ionic liquid
An ionic liquid (IL) is a salt in the liquid state. In some contexts, the term has been restricted to salts whose melting point is below some arbitrary temperature, such as 100 °C (212 °F). While ordinary liquids such as water and gasoline are predominantly made of electrically neutral molecules, ionic liquids are largely made of ions and short-lived ion pairs. These substances are variously called liquid electrolytes, ionic melts, ionic fluids, fused salts, liquid salts, or ionic glasses. Ionic liquids have many applications, such as powerful solvents and electrically conducting fluids (electrolytes). Salts that are liquid at near-ambient temperature are important for electric battery applications, and have been used as sealants due to their very low vapor pressure.Any salt that melts without decomposing or vaporizing usually yields an ionic liquid. Sodium chloride (NaCl), for example, melts at 801 °C (1,474 °F) into a liquid that consists largely of sodium cations (Na+) and chloride anions (Cl−). Conversely, when an ionic liquid is cooled, it often forms an ionic solid—which may be either crystalline or glassy.The ionic bond is usually stronger than the Van der Waals forces between the molecules of ordinary liquids. For that reason, common salts tend to melt at higher temperatures than other solid molecules. Some salts are liquid at or below room temperature. Examples include compounds based on the 1-Ethyl-3-methylimidazolium (EMIM) cation and include: EMIM:Cl, EMIM dicyanamide, (C2H5)(CH3)C3H3N+2·N(CN)−2, that melts at −21 °C (−6 °F); and 1-butyl-3,5-dimethylpyridinium bromide which becomes a glass below −24 °C (−11 °F).Low-temperature ionic liquids can be compared to ionic solutions, liquids that contain both ions and neutral molecules, and in particular to the so-called deep eutectic solvents, mixtures of ionic and non-ionic solid substances which have much lower melting points than the pure compounds. Certain mixtures of nitrate salts can have melting points below 100 °C.The term ""ionic liquid"" in the general sense was used as early as 1943.