Chemistry Reviewer Notes, Study notes of Chemistry

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Module 1: Properties of Matter Properties of Substances Electrical Conductors. Materials that can transmit the flow of energy. They have freely moving electrons that can transfer thermal energy quickly and easily. Examples: Aluminum, Copper, Gold Electrical Insulators. Materials that prevent the flow of energy. They prevent electrons from moving through them. Examples: Rubber tires, Wood, Plastic battle Density. It depends on the temperature and pressure when it is measured. Examples: Copper wire, Water, Gasoline Acidity. Acidic solutions have a greater concentration of hydrogen ions, and basic solutions have a lower concentration of hydroxide ions. Examples: Soda, Coffee Flammability. Flammable materials largely depend on the chemical elements present in their structures. The presence of more carbon generally results in more flammable material. Example Alcohol, Wood Reactivity. Is the substances tendency to undergo a chemical reaction, either by itself or with other materials, and to release energy. Reactive can be hazardous and poisonous when caused to react by heat, pressure, shock, friction, catalyst, contact with air or water. **Malleability.** Ability of a material to be pressed, hammered, or rolled into thin sheets without breaking the matter. **Ductility.** Ability of a material to be stretched under stress and converted into thin wires. Example: Copper, Iron wire, Aluminum wire **Solubility**. Ability of a substance to be dissolved (solute) in a given substance (solvent). Example: Solute – coffee, milk & sugar Solvent - water **Boiling Point**. Is the temperature at which a substance changes from a liquid into gas. **Melting Point**. Is the temperature at which a material changes from solid into a liquid. **Polarity.** Is the way at which an atom forms a covalent bond. This relates to solubility, boiling and melting points, and intermolecular attractions between molecules. **Elasticity**. It is the tendency of a material to return to its original form or shape after being stretched. Example: Spring tor, Rubber band **Corrosiveness**. A property of a material that causes gradual destruction by a chemical reaction such as strong acids, oxidizers, and bases. _Types of Properties of Matter_ **Physical Property** is a property of matter that is measured without changing a substances chemical identity. Types of Physical property Intensive Property is a matter that is independent of the amount of a substance. Extensive Property is a matter that depends on the amount of the substance. Chemical Property is a property of a matter that is measured only by changing the substance`s identity.

Module 2: Consumer Products The Chemistry behind some Consumer Products Alcohol-based and Alcohol – free Hand Sanitizer Alcohol-based sanitizer contains 60-65% alcohol. flammable, cause potential toxicity hazards once it is ingested and dryness is A lcohol–free hand sanitizer (benzalkonium chloride). do not dry out hands, they have less threat, low fire hazard. Surgical facemask, N95 mask and Fabric Mask citric acid, zinc, and copper are the components Latex, Nitrile and Vinyl Gloves. Gloves would be a convenient way to minimize contamination and keep our hands clean. Soaps and Detergents clothes. Soap is produced sodium hydroxide (NaOH) or potassium hydroxide (KOH) with animal fatsor vegetable oilsin the process called saponification. Toothpaste. Sodium Fluoride (NaF) keeps the teeth clean and replaces the lost calcium and phosphorous called remineralization. Triclosan that works as antifungal and antibiotic preventing gingivitis. Module 3: Separation Techniques of Mixtures Separation Techniques of Mixtures Magnetic separation is a technique in separating components of a mixture by using magnet to attract magnetic materials and detaches thenonmetallic materials. Evaporation is another separation technique used in homogeneous mixtures and it typically involves heating the mixture until no more liquid remains and what is left is the residue. Decantation is allowing a mixture of solid and liquid or two immiscible liquids to settle and separate using their differences in densities. Sedimentation is involved in this technique where heavy particles settle down at the bottom of the mixture. Gravity Filtration is one of the types of filtration that is used in chemical laboratories. The fluid that passes through the filter is called filtrate. In this type of separation technique, filter paper, funnel, stirrer, and beaker are used. Distillation is effective in removing organic compounds that vary on solubility and boiling point. It is a separation technique for a mixture of two miscible liquids with a sufficient difference in their boiling points.

Module 4: Atoms and Their Isotopes Nucleus- Atoms contain a central portion. Inside the nucleus are protonsand neutrons. Protons and neutrons are often called nucleons. Protons (p+) and neutrons (n^0 ) are neutral. Whirling about the nucleus are particles called electrons (e-) ATOMIC NUMBER vs. MASS NUMBER Atomic number (Z) =(p+)=(e-) Mass number (A) =(p+) +(n^0 ) Isotopes are different version of the same element.

• same Atomic #, Protons Electrons
• different Masses and Neutrons Radioactive decay is the process in which an unstable atomic nucleus spontaneously loses energy by emitting ionizing particles and radiation. Parent nuclide - Daughter nuclide- decayor loss of energy transforming to an atom MODES OF RADIOACTIVE DECAY Alpha emission (α) is a low- penetrating emission. Beta particles (ß-) are emissions having medium level penetration. Positron emission (ß+) is the positive counterpart of an electron emission. Electron capture As a result of electron capture, a proton is converted into a neutron. Gamma (У) emissions as they are commonly referred to, are highly penetrating and dangerous emissions. Module 5: Chemical Formulas, Structural Formulas, and Models of Ionic Compounds Chemical formula indicates the element and their proportion in compound. Two importance of Chemical formula 1.the elements that make up the compound (element symbols); and 2.the number of atoms of each element that are present in a compound (numerical subscripts). IONIC COMPOUND. an element composed of atoms that readily lose electrons(a metal) reacts with an element composed of atoms that readily gain electrons (a nonmetal) Common Cations - metals lose enough electrons Common Anions - nonmetals, tend to gain electrons Ionic compounds are of two types: Binary and Ternary. BINARY IONIC COMPOUNDS composed of ions of two different elements-one of which is a metal and the other a nonmetal. TERNARY/TERTIARY IONIC COMPOUNDS– compounds composed of three or more elements with one type of cation and one type of anion involved. STRUCTURAL FORMULA

Module 6: Naming Ionic Compounds Ionic compound 1 M 1 NM Covalent compound 2 nonmetal Rule 1. When writing a chemical formula for ionic compounds, write the metal element first. Rule 2. For cations, the name of the element is unchanged. Rule 3. For anions, the name of the element is modified by the suffix –ide. Rule 4. The polyatomic cation NH4+ is named as ammonium. Rule 5. Several anions are polyatomic and are named based on the atomic constituents and the suffix – ide. Rule 6. A number of polyatomic anions containing oxygen atoms are named based on the root word of the central atom and the suffix –ate for the one with more oxygen atoms and –ite for the one with less oxygen atom. Module 7: Chemical Formulas, Structural Formulas, and Models of Covalent Compounds MOLECULAR FORMULA – shows the actual number of atoms of each element in a molecule of the compound.

1. BINARY COVALENT – composed of two different elements – a nonmetal and another nonmetal. Numerical Prefixes for Binary Covalent Compounds
2. BINARY ACIDS – comprised of hydrogen and one other nonmetallic element.
3. TERNARY ACIDS (oxyacids) – contains three or more elements
   4. BASES – substances that increase OH- ions in an aqueous solution. Examples: Lithium and hydroxide – LiOH Module 8: Naming Covalent Compounds -For the first element, start with the element name -For the second element, start with the –ide name -Use prefixes to show how many atoms of each types there are -Do not use “mono” in the first element F- fluoride Cl -chloride Br-bromide I- iodine O- oxide S- sulfur N- nitride P-phosphide Example: