Results for "NH3"

Bài toán hiệu suất tổng hợp NH3

chemical test when adding NaOH and NH3

Reactions of Transition Metal Complexes

Part II. Multiple choice, continued (3 points each). Name:__________________ Please circle your answer. There is only one correct answer to each question. 52. A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is __________ atm. A) 0.60 B) 1.5 C) 1.0 D) 0.35 53. Of the following gases, _____________ will have the greatest rate of effusion at a given temperature. A) NH3 B) CH4 C) Ar D) HCl 54. Which noble gas is expected to show the largest deviations from the ideal gas behavior? A) helium B) neon C) argon D) krypton 55. Together, liquids and solids constitute _______ phases of matter. A) the compressible B) the fluid C) the condensed D) the disordered 56. What is the predominant intermolecular force in liquid CBr4? A) dispersion B) dipole-dipole C) ion-dipole D) hydrogen bonds 57. Of the following substances, ____________ has the highest boiling point. A) H2O B) CO2 C) CH4 D) Kr 58. Of the following substances, ____________ has the lowest boiling point. A) Kr B) Ar C) Ne D) Xe 59. What is the predominant intermolecular force in liquid HBr? A) dispersion B) dipole-dipole C) ion-dipole D) hydrogen bonds 60. The total pressure of a mixture of O2 and N2 is 730 torr. The partial pressure of N2 is 0.78 atm. The partial pressure of O2 is A) 0.18 atm B) 0.22 atm C) 0.26 atm D) 0.78 atm

Multiple choice, continued (3 points each). Name:__________________ Please circle your answer. There is only one correct answer to each question. 36. How many different resonance structures can be drawn for the molecule SO3 without having to violate the octet rule on the sulfur atom? A) 5 B) 4 C) 3 D) 2 37. The central atom in _______ does not violate the octet rule. A) CF4 B) KrF2 C) SF4 D) XeF4 38. For a given arrangement of ions, the lattice energy increases as ionic radius _________ and as ionic charge __________. A) increases, increases B) decreases, decreases C) increases, decreases D) decreases, increases 39. Of the molecules below, only ________ is nonpolar. A) HCl B) NH3 C) SO2 D) CO2 40. Using the table of bond dissociation energies, ∆H for the reaction 2HCl (g) + F2 (g) à 2HF (g) + Cl2 (g) is __________ kJ. Bond D (kJ/mol) H – Cl 431 F – F 155 H – F 567 Cl – Cl 242 A) –359 B) -223 C) 359 D) 223 41. Considering its Lewis structure, the electron-domain geometry of oxygen in OF2 is ___________. A) trigonal planar B) trigonal bipyramidal C) octahedral D) tetrahedral 42. The electron-domain geometry and the molecular geometry of ammonia, NH3, are __________ and __________, respectively. A) tetrahedral, trigonal pyramidal B) tetrahedral, trigonal planar C) bent, bent D) trigonal planar, bent

Ppt with Nh3 and NaOH

Precipitate colours with NaOh and Nh3

Identifying aqueous cations using NaOH or NH3 solution

NH3 uptake and Amino Acid Syn

Chapter 4 The Effects of Chemical Reactions. • Introduction to Chemical Reactions. - Chemical reaction: a process in which one or more substances change into one or more new substances. - Clues that a chemical reaction has occurred : 1. Color change Example: two colorless aqueous solutions mix together to produce a bright yellow precipitate. 2. A precipitate (solid) is formed when mixing two solutions together. 3. Gas formation. Bubbles of gas (effervescence) are produced when mixing substances together (solid – liquid or aqueous – aqueous ….) 4. Heat is produced. - Chemical reactions are described by using word equations or chemical equations. - Chemical equations need to be balanced when written because it shows the correct proportions (amounts) of chemicals in a reaction. - A balanced chemical equation has equal number of atoms of each element in the reactants (left hand side) and the products (right hand side). - Exercise: Balance the following equations. a) KClO3→KCl + O2 b) Na2O + H2O NaOH c) Cu + AgNO3 Cu(NO3)2 + Ag d) C3H7OH + O2 CO2 + H2O • Synthesis and Decomposition Reactions. Synthesis: Two or more substances (elements and / or compounds) combine to form one larger compound. General pattern: A + B → C Examples: N2 + 3 H2 → 2 NH3 CaO + CO2 → CaCO3 2 P + 3 Cl2 → 2 PCl3 Decomposition: This is opposite to synthesis; that is, one large compound breaks down (decomposes) into 2 or more simpler substances. Example: 2 KClO3 → 2 KCl + 3 O2 General pattern: R → S + T Remark: Usually decomposition happens due to heat or electricity. - Predicting the product of decomposition or synthesis reactions. 2 AlCl3 (s) → 2 Al (s) + 3 Cl2 (g) Zn (s) + S (s) → ZnS (s) 2 Zn (s) + O2 (g) → 2 ZnO(s) - Single Displacement (Replacement) Reactions. Definition: A reaction in which an element displaces (replaces) another element in a compound, producing a new compound and a new element. General pattern: A + BC → AC + B Example: Mg (s) + CuSO4 (aq) → MgSO4 (aq) + Cu (s) Zn (s) + 2 AgNO3 (aq) → Zn(NO3)2 (aq) + 2 Ag (s) Fe (s) + MgCl2 (aq) → no reaction. Remark: The element that displaces the other element in a compound must be more reactive (active) than that element, otherwise no reaction takes place. In the general pattern above, A should be more reactive than B for the reaction to proceed. The following reactivity (activity) series lists the chemical strength (reactivity) of the metals in order from the more reactive to the less reactive. KPlease stop calling my amazing zebra in the long Nahungry class. sorry !! Ca Mg Al Zn Fe Sn Pb H Cu Ag Examples of single displacement reactions : 2 Al (s) + 3 CuSO4 (aq) → Al2(SO4)3 (aq) + 3 Cu (s) Sn (s) + Zn(NO3)2 (aq) → no reaction Exercise: Complete and balance the following equations. If there is no reaction occurring write no reaction. a) 2 Al (s) + 6 HCl (aq) → 2 AlCl3 (aq) + 3 H2 (g) b) Cu (s) + H2SO4 (aq) → no reaction c) 2 AlCl3 (aq) + 3 Ca (s) → 3 CaCl2 (aq) + 2 Al (s) d) Mg (s) + 2 HNO3 (aq) → Mg(NO3)2 (aq) + H2(g) - Reactivity of halogens decreases down the group. F2> Cl2> Br2> I2 The reactions taking place for the halogens or their compounds are in solution (aqueous) Examples: Cl2 (aq) + 2 KBr (aq) → 2 KCl (aq) + Br2 (l) Cl2 (aq) + NaF (aq) → no reaction. Exercise: F2 (aq) + 2 LiCl (aq) → 2 LiF (aq) + Cl2 (g) I2 (aq) + NaCl (aq) → no reaction • Double displacement reactions. - Definition: A reaction in which two compounds mix together and an exchange of ions (elements) occurs which results in the formation of 2 new compounds. - General pattern: AB + CD → AD + CB - Solubility: the amount of solute that dissolves in a given amount of solvent at a given temperature. - When we say a substance is soluble, it means it dissolves in water; whereas if it is insoluble it means it doesn’t dissolve in water. - The compound in a reaction that is soluble is in aqueous (aq) phase, whereas the compound which is insoluble is in the solid state (s). - The solid which is formed in a double displacement reaction is called the precipitate and it is insoluble. - Solubility rules (used in double displacement reactions). 1. All alkali metal ions and ammonium ion (NH4+) are soluble. 2. All nitrates (NO3-) are soluble. 3. All sulfates (SO4-2) are solubleexceptwith Ba+2 , Pb+2 , Ca+2 , Sr+2 , Ag+ . 4. All chlorides, bromides and iodides(Cl-, Br-, I-) aresolubleexcept with Ag+ , Pb+2 , Hg+, Cu+ 5. All OH- are insolubleexceptwith rule 1, and Ba+2 and Sr+2 . 6. All oxides (O2-), sulfides (S2-), sulfites (SO32-), carbonates (CO32-), phosphates (PO43-) are insoluble except with rule 1 Remark: If all compounds formed in a double displacement reaction are soluble (aqueous) then no reaction takes place. Exercise: State whether each of the following compounds is soluble or insoluble ? Na2SO4 : Fe(NO3)2: LiOH: ZnSO4: PbBr2: BaSO4: Mg(OH)2: PbO: NH4Cl: Na2S: Cu(OH)2: KF: Exercise: Complete and balance the following chemical equations: - KNO3 (aq) + NaCl (aq) → - LiCl (aq) + AgNO3 (aq) → - Zn (s) + FeSO4 (aq) → - NaOH (aq) + CuCl2 (aq) → - ZnCl2 (aq) + Na3PO4 (aq) → - Pb(NO3)2 (aq) + K2S (aq) → • Net ionic equation: a chemical equation which shows ONLY the ions that are involved in the formation of the precipitate (solid). Examples: Pb+2 (aq) + S-2 (aq) → PbS (s) Ag+ (aq) + Cl- (aq) → AgCl (s) Cu+2 (aq) + 2 OH- (aq) → Cu(OH)2 (s) • Full ionic equation: an equation which shows All the ions in the soluble (aqueous compounds) in both reactants and products. Example: - 2 NaOH (aq) + CuCl2 (aq) → 2 NaCl (aq) + Cu(OH)2 (s) 2 Na+ (aq) + 2 OH- (aq) + Cu+2 (aq) + 2 Cl- (aq) → 2 Na+ (aq) + 2 Cl- (aq) + Cu(OH)2 (s) - 3 ZnCl2 (aq) + 2 Na3PO4 (aq) → Zn3(PO4)2 (s) + 6 NaCl (aq) Full ionicequation: 3 Zn+2(aq) + 6 Cl-(aq) + 6 Na+ (aq) + 2 PO4-3 (aq) → Zn3(PO4)2 (s) + 6 Na+ (aq) + 6 Cl- (aq) Net ionic equation: 3 Zn+2 (aq) + 2 PO4-3 (aq) → Zn3(PO4)2 (s) Exercise: Complete and balance the following equation, then write full ionic and net ionic equations for the reaction. Pb(NO3)2 (aq) + 2 NaI (aq) → Full ionic equation: Net ionic equation: Spectator ions: the ions that are not involved in the formation of the precipitate (solid). Note that the spectator ions appear on both sides of the full ionic equation. For example, in the above reaction, Na+ (sodium ions) and NO3- (nitrate ions) are the spectator ions. Exercise: Complete and balance the following equation, then write the net ionic equation and identify the spectator ions. BaCl2 (aq) + K2SO4 (aq) → Net ionic equation: Ba+2 (aq) + SO4-2 (aq) → Spectator ions: - Combustion reaction is a special type of (synthesis) reaction in which the substance reacts with (burns in) oxygen. Examples: C(s) + O2(g) → CO2(g) • Production of gases (lab scale): 1. CO2 2. SO2 3. H2 4. H2S (hydrogen sulfide) 5. NH3 (ammonia) General pattern of the chemical reactions to produce the above gases: 1. Metal carbonate + acid → CO2 Example: Na2CO3 (aq) + 2 HCl (aq) → 2 NaCl(aq) + CO2(g) + H2O(l) 2. Metal sulfite + acid → SO2 K2SO3 (aq) + 2 HCl (aq) → 2 KCl(aq) + SO2(g) + H2O(l) 3. Metal + acid → H2 Remark: This is a single displacement reaction therefore the metal used in the reaction should be higher in the reactivity series than hydrogen. Zn (s) + 2 HCl (aq) → ZnCl2 (aq) + H2(g) 4. Metal sulfide + acid → H2S Na2S (aq) + 2 HCl (aq) → 2 NaCl (aq) + H2S (g) 5. Ammonium compound + base (alkaline solution) → NH3 NH4Cl (aq) + NaOH (aq) → NaCl (aq) + NH3 (g) + H2O (l) Exercise: Write the net ionic equations for each of the above 5 reactions. Answers 1. 2 H+ (aq) + CO3-2(aq) → CO2(g) + H2O (l) 2. 2 H+ (aq) + SO3-2(aq) → SO2(g) + H2O (l) 3. Zn(s) + 2 H+(aq) → Zn+2(aq) + H2(g) 4. 2H+ (aq) + S-2 (aq) → H2S (g)

NH3

Se merece más (NH3- U5) frases para practicar

NH3 - Una experiencia inolvidable - PC

1. ĐL NH3 bằng dd HCl 0,1N

NH3/NH4/HNO3

Lect 20. NH3 uptake and aa synthesis

Reactions of TM ions with NaOH, Na2CO3 and NH3

Organic Chemistry – branch of chemistry which deals with study of carbon containing compounds their properties , composition, structure , reactions and preparations. Organic compounds – are carbon containing compounds with the exception of carbon dioxide, carbonates and bicarbonate Inorganic Chemistry – branch of chemistry which deals with the study of all elements and compounds other than organic compounds Comparison of the properties of most Organic and Inorganic compounds Properties Organic Inorganic Flammable Yes No Melting point Low High Boiling point Low Hogh Solubility in water Insoluble Soluble Solubility in non polar solvent Soluble Insoluble Type of bond Covalent Ionic bond Reaction occurs between Molecule Ions Atoms per molecule Many Few Structure Complex Simple Electrolyte No Electrolyte Organic compounds A. Hydrocarbon -compounds that contains only carbon and hydrogen 1. Saturated - contains single bond ; Example Alkane ( CnH2n+2) 2. Unsaturated – contains double or triple bond. a. Alkene – contains double bond ( CnH2n ) b. Alkyne - Contains triple bond (CnHn-2 ) c. Aromatic Hydrocarbon - hydrocarbon that contains benzene ring B. Hydrocarbon derivative – compounds that contains carbon and hydrogen and other element such O, N, P,S, halogens. 1. Alcohol - ROH organic compound produced by hydration of alkene 2. Ether - ROR - prepared by dehydration of alcohol 3. Aldehyde – RCHO – prepared by oxidation of primary alcohol 4. Ketone – RCOR – prepared by oxidation of secondary alcohol 5. Carboxylic Acid - RCOOH – prepared by oxidation of aldehyde 6. Amine - organic compound derived from ammonia ( NH3) a. Primary Amine –R NH2 b. Secondary Amine – R2NH c. Tertiary Carbon – R3N 7. Amide – RCONH2 – organic compound prepared by the reaction of carboxylic acid ammonia. 8. Ester – RCOOR – Organic compounds prepared by the reaction of carboxylic acid and alcohol Structural formula - two dimensional structural representation that shows how the various atoms in a molecule are bonded to each other a. Expanded structural formula - show all atoms in a molecules and all bonds connecting them. b. Condensed structural formula – uses groupings of atom in which central atoms and the atoms connected to them are written in a group. c. Skeletal structural formula - show the arrangement and bonding of carbon atoms present in an organic molecule but does not show the hydrogen atom attached to the carbon atom - d. Line angle structural formula - structural representation in which a line represent a carbon-carbon bond and a carbon atom is understood to be present at every point where two lines meet and at the end of the line. Classification of Carbon Atoms 1. Primary Carbon - carbon atom in an organic molecule that is directly bonded to one carbon one other carbon atom. Ex. CH3- CH3 10 1O 2. Secondary carbon atom – is a carbon atom in an organic molecule that is directly attached to two 3. Tertiary carbon - carbon atom in an organic molecule that is directly attached to three other carbon atoms. 4. Quarternary carbon atom - is a carbon atom in an organic molecule that is directly attached to four other carbon atoms. Alkyl group – group of atom that would be obtained by removing a hydrogen atom from an alkane Substituent – is an atom or group of atoms attached to a chain or ring of carbon atoms. Alkane - Saturated hydrocarbon that contains single bond Rules in naming alkane 1. Choose the longest continuous chain as your parent chain 2. Locate the position of the substituent starting from the carbon nearest to it. 3. If there are two or more the same substituents , use the Greek prefixes such as di, tri , tetra, etc. 4. If there are different substituents, write the name in alphabetical order, 5. Use commas between numbers and hyphen between number and letter. Isomer – compounds with same molecular formula but different structural formula CH3 – CH2 – CH2 – CH2- CH3 CH3 – CH2 – CH – CH3 CH3 CH3 CH3 – C – CH3 CH3 Cycloalkane – saturated hydrocarbon in which carbon atoms connected to one another in a cycl (ring) arrangement are present. The simplest cycloalkane is cyclopropane.

Aqueous cations test with NaOH and NH3

NH3/U1 Perspectivas de Arte