CHEM

• The objectives of the course include performing dimensional analysis in basic calculations, solving problems involving density and concentrations of solutions, and describing the methods and steps involved in quantitative analysis.
• The course covers fundamental concepts in analytical chemistry such as units of measurement, dimensional analysis, recall on general chemistry principles, density of solutions, solution concentration, and general steps in quantitative and qualitative analysis.
• Traditional branches of chemistry include chemistry, which deals with the study of the structure of matter and changes it undergoes, and analytical chemistry, which deals with the identification of compounds and mixtures and the determination of the proportions of the constituents.
• On successful completion of the course, students will be able to develop an understanding of the range and uses of analytical methods in chemistry, establish an appreciation of the role of chemistry in quantitative analysis, employ measurement and problem solving for analytical tasks for different fields of interest, and provide an understanding of chemical methods employed for elemental and compound analysis.
• The International System of Units (SI) is the most common system in measuring matter and conversion to non-SI units vice versa is essential.
• The basic SI units can be expressed as fractions and multiples of basic units by using a set of simple prefixes.
• Mass (m) is a measure of the quantity of matter in an object.
• Weight (w) is the force that gravity exerts on an object given by the formula w = mass x acceleration due to gravity and is a derived unit.
• Length (l) is the measurement or extent of something from end to end.
• Volume (V) is the amount of space occupied by a three-dimensional figure as measured in cubic units and is a derived unit.
• Sulfuric acid, barium chloride, sulfurous acid, sodium acetate, phosphoric acid, acetic acid, potassium permanganate, plumbous oxide, sodium carbonate, ferric hydroxide.
• Molar Mass (MW) is the total mass of all the atoms in grams that make a mole of a particular molecule.
• Avogadro’s Number (NA) is the numbers of particles required such that the mass of a substance will be equal to the substance’s atomic mass.
• AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq) is an example of a double-displacement reaction.
• Double-displacement reaction involves the parts of two ionic compounds being exchanged, resulting in two new compounds.
• Exercise - Molar Mass: Compute for the molar mass of the following compounds.
• Molar Mass (M) is the mass in grams of one mole of a particular element/compound – g/mol.
• Molar mass (M) is the total mass of all the atoms in grams that make a mole of a particular molecule.
• Mass of 5 mol of sulfuric acid, moles of 1 kg of sulfurous acid, moles of 15 g of phosphoric acid, mass of 0.055 mol of potassium permanganate, moles of 10.29 lb sodium carbonate.
• Molar Mass (MW) is the mass in grams of one mole of a particular element/compound expressed in g/mol.
• Molar mass (g/mol) is the atomic mass expressed in grams.
• Precipitation reaction forms Lead (II) iodide.
• Mole (mol) is the numbers of particles required such that the mass of a substance will be equal to the substance’s atomic mass.
• Molecular mass/weight (MW) is the total mass of all atoms in amu present in the compound.
• A positive ion, or cation, is an atom or group of atoms that has a net positive charge.
• The density of the metal can be calculated by dividing the total mass by the volume of the container.
• The forces that hold atoms together in compounds are called chemical bonds.
• Examples of molecules that contain covalent bonds are hydrogen (H2), water (H2O), oxygen (O2), ammonia (NH3), and methane (CH4).
• A covalent bond forms when the difference between the electronegativities of two atoms is too small for an electron transfer to occur to form ions.
• A methane molecule can be represented as a molecular formula, a structural formula, a ball-and-stick model, and a space-filling model.
• Carbon and hydrogen atoms are represented by black and white spheres, respectively, in a methane molecule.
• An ion, or anion, is an atom or group of atoms that has a net negative charge.
• Molecules formed by chemical bonding are named in terms of chemical formula, in which the symbols for the elements are used to indicate the types of atoms present.
• In a second experiment, 25.0920 g of metal beads were put into the container and the flask was again filled to the 25.00-mL mark.
• There are two types of chemical bonding: covalent bonding, which results from sharing one or more electron pairs between two atoms, and ionic bonding, which results from electrostatic interactions among ions, often resulting from the net transfer of one or more electrons from one atom or group of atoms to another.
• A calibrated flask was filled to the 25.00-mL mark with ethyl alcohol and it was found to have a mass of 19.7325 g.
• The total mass of the metal plus the alcohol was 43.0725 g.
• An ionic compound is formed when a positive ion and a negative ion attract each other.
• Electronegativity is the tendency for an atom of a given chemical element to attract shared electrons when forming a chemical bond.
• Elements can be categorized as metals, non-metals, and metalloids based on their properties.