Chemistry Unit Test Review PDF

Chemistry Unit Test Review Chapter 5 - Matter is anything that takes up mass and occupies space. All matter is made of tiny particles that have empty space between them. - Particles are in constant motion and move faster as the temperature increases. - Solid, Liquid, Gas...

Chemistry Unit Test Review Chapter 5 - Matter is anything that takes up mass and occupies space. All matter is made of tiny particles that have empty space between them. - Particles are in constant motion and move faster as the temperature increases. - Solid, Liquid, Gas - Thermal energy heats up atoms, which crash into each other, which makes the atoms move. - The Transfer of energy always happens from hot surfaces to cool surfaces. Mixtures - Mixture - a substance that is made up of at least two different types of particles. (Ex. Granola Bar) - Mechanical Mixture - A mixture in which you can distinguish between different types of matter. (Ex. Cereal) - Solution - An even mixture of two or more substances that can’t be seen. (Ex. Apple Juice) - Pure Substance - A substance that is made up of only one type of particle. - Alloy - a solid solution of two or more metals. (Ex. Stainless Steel, Bronze) Qualitative properties: are properties that are observed and can generally not be measured with a numerical result. Quantitative properties: are properties of a physical system which exists in a range of values corresponding with a number Physical Properties - Is a substance that helps to identify it by the way it looks. Using Senses - Hear, Touch, Taste, Smell, Sight - Colour - Odour - Taste - Texture - Lustre - Shininess or dullness  - Optical Clarity - The ability to let light through. (Transparent, Translucent and Opaque) - Brittleness - Breakability or flexibility. (Glass is brittle and clay is flexible.) - Viscosity - How easily a liquid flows. (Syrup is more viscous than water) - Hardness - How Hard a solid is. - Malleability - How well an object can be bent or hammered into different shapes. - Ductility - Is how well an object can be made into wiring. - Electrical Conductivity - The ability of a substance to allow an electric current to pass through it. (Copper wires have high conductivity) - Solubility - How well a substance can dissolve in a liquid. - Melting and Boiling Point - Temperature at which a substance changes state. Chemical Properties - Are determined when the composition of the substance is altered. 1. Change of Colour 2. Change of Odour 3. Forms Bubbles 4. New Solids being formed 5. Heat or light being released. Characteristic Physical Property - a characteristic property that can be determined without modifying the nature of a substance. (Ex. Density, Pure Substance, Melting Point, Etc.) Density: amount of matter per unit volume of that matter. (Mass/Volume) Formula: M D/V Volume: Space Occupied by an Object. Mass: the amount of matter that makes up an object. Water Density: 997 kg/m³ If other densities are less dense, it will float, if it is denser, then it will sink. G.R.A.S.P Method: Given, Required, Analysis, Solution and Paraphrase Chapter 6 Atoms: are the basic particles of the chemical elements Elements: a chemical substance that cannot be broken down into other substances by chemical reactions. Compound: a substance made from two or more different elements that have been chemically joined Subatomic Particle: a particle smaller than an atom (e.g., a neutron) Reactant: a substance that takes part in and undergoes change during a reaction. Formula: a mathematical relationship or rule expressed in symbols. Product: is a substance that is present at the end of a chemical reaction. Pure Substances: can be classified as a elements or compounds Isotope: each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons, which differ in atomic mass Protons: A particle that lives in the nucleus with a positive charge Electrons: A particle that orbits the nucleus with a negative charge Neutrons: A particle that lives in the nucleus with a neutral charge Valence electrons: The electrons in the outermost orbital of an atom. History of the Atom Democritus - All matter can be divided into smaller and smaller pieces until a single indivisible particle is reached. (Atom) Aristotle - All matter is made up of four basic substances, Earth, Water, Air and Fire. John Dalton - Revived Democritus’ theory. All matter is made up of tiny particles called Atoms. Experiment - Billiard Ball Model J.J. Thomson - Discovered extremely small negatively charged particles called Electrons Experiment - Plum Pudding Model Ernest Rutherford: Through an experiment that fired small, positively charged particles at a thin piece of gold foil. Nucleus of an atom contains positively charged particles called Protons. Experiment - The Gold Foil Experiment James Chadwick: Revised Rutherford’s theory and proposed that the nucleus contains protons and neutral particles called Neutrons. Niels Bohr: Studied the Hydrogen atom. States electrons orbit the nucleus. Each orbit can hold a maximum number of electrons. Experiment - Bohr-Rutherford Diagram Periodic Table - 118 elements - Our version of the periodic table was developed by Dmitri Mendeleev.  - Periods: Horizontal rows of the periodic table. They represent the number of orbitals the elements of on a Bohr- Rutherford Diagram - Groups: Vertical columns of the periodic table. They represent the number of valence electrons on a Bohr- Rutherford diagram. - On the left side, the more down you go the more reactive the elements get. 👆 - On the right side, the more up you go the more reactive the elements get. - Different Families of the periodic table Bohr - Rutherford Diagram Standard Atomic Notation (S.A.N) Chapter 7 - Molecule: made up of one or more atoms - Molecular/Covalent Compounds: pure substances made up of two or more non- metal atoms. When non-metals combine with other non-metallic atoms. - Diatomic Molecules: a molecule composed of two of the same atom. (Ex. Nitrogen, Oxygen, Iodine, Fluorine) - Ion - a charged atom - Ionic Compounds: Composed of charged particles called ions. Can be positively or negatively charged. Mixture of non-metals and metals. (cations or anions) - Cations: is formed when a metal loses one more electrons - Anions: is formed when a non-metal gains one or more electron - Subscript: a small-sized number on the bottom right of the symbol. It refers to the number of atoms of the element. - Metals tend to lose electrons, which are Cations - Non-Metals tend to gain electrons, which are Anions - When an atom LOSES an electron, it has one more proton than electrons and therefore has a net POSITIVE CHARGE. - When an atom GAINS an electron, it has one more electron CHARGE. - Ionic Bond - formed between two or more atoms by the transfer of one or more electrons between atoms. When an atom Loses an electron, it has one more proton than electron and therefore has a Positive Charge. When an atom Gains an electron, it has one more electron than protons and therefore has a Negative Charge Counting Atoms Periodic Table Charges