Long Test 1.1 Science Reviewer 9 PDF

LONG TEST 1.1 SCIENCE REVIEWER 9 ___________________________________________________________________ T1.1: Introduction to Chemistry PROPERTIES OF MATTER ➔ Characteristics that allow...

LONG TEST 1.1 SCIENCE REVIEWER 9 ___________________________________________________________________ T1.1: Introduction to Chemistry PROPERTIES OF MATTER ➔ Characteristics that allow us to CHEMISTRY recognize matter and ➔ Deals with properties, distinguish them from the other composition, structure, and substances. changes that material undergo. Physical Properties BRANCHES OF CHEMISTRY ➔ It is a characteristic that we can observe and measure without Organic Chemistry changing the composition of a ➔ A branch of chemistry which deals substance. with the study of carbon compounds. KINDS OF PHYSICAL PROPERTIES ➔ Carbon is capable of forming long C - C chains called catenation. Intensive Property ➔ Does not depend on the amount Inorganic Chemistry of substance being examined ➔ It deals with the study of inorganic Examples: compounds. Boiling Point ➔ Inorganic compounds are Color compounds which do not contain Temperature carbon-hydrogen bonds. Luster Hardness Biochemistry ➔ It deals with the study of Extensive Property chemical processes inside the ➔ Depends on the amount of biological system. substance Examples: Analytical Chemistry Volume ➔ It deals with qualitative and Mass quantitative methods to analyze Size properties of matter. Weight Length Physical Chemistry ➔ It is concerned with the application Chemical Properties of the techniques and theories of ➔ Chemical properties are physics to the study of chemical descriptions of the ability of a systems. substance to undergo a chemical change. T1.2: Properties of Matter Examples: Flammability MATTER Corrosiveness ➔ Anything that occupies space and Acidity has mass. Toxicity ➔ Mass represents the amount of Chemical Reactivity matter Tarnish MJT & SMB || 1  LONG TEST 1.1 SCIENCE REVIEWER 9 ___________________________________________________________________ CHANGES IN MATTER LIQUID ➔ No fixed shape Physical Changes ➔ Takes shape of filled portion of the ➔ It is a process that changes the container physical properties of a ➔ Can be poured substance without changing its chemical composition. GAS ➔ Changes in physical state are ➔ No fixed shape physical changes. ➔ Takes shape of the container Examples: ➔ Fills container Melting Evaporation IN MOLECULAR LEVEL Freezing ➔ A particle is an extremely tiny Condensation piece of matter, and scientists believe that everything in the Chemical Changes universe is made up of particles. ➔ It is a process where one or more ➔ Particles can range in size, from substances are converted into atoms or molecules, or to much one or more new substances. more smaller submicroscopic ➔ Also called a chemical reaction. particles like electrons. Examples: Permanent change in color Kinetic Molecular Theory (KMT) Sudden change in temperature ➔ It helps us interpret the Formation of precipitate microscopic properties of solids, Evolution of gas liquids and gases. Change in odor ➔ According to the theory, all matter Bubbling consists of extremely tiny particles, which are in constant T1.3: States of Matter motion. MATTER MATTERS Heated ➔ Can be classified based on physical state and composition Cooled Kinetic Energy (KE) OBSERVABLE PROPERTIES OF THE ➔ The energy of the moving object THREE STATES If the speed of the object increases, its KE increases. SOLID If the speed of the object ➔ Fixed shape decreases, its KE decreases. ➔ Shape not set by container ➔ Shape remains rigid When object is heated or cooled When particles are heated, they move faster MJT & SMB || 2  LONG TEST 1.1 SCIENCE REVIEWER 9 ___________________________________________________________________ When they are cooled, they move WATER EXISTS IN THREE DIFFERENT slower PHASES Effect on kinetic energy ➔ The amount of energy affects the Particles have more kinetic arrangement and rate of energy movement of atoms or molecules Particles have less kinetic energy in matter, which leads to the different phase changes. IN MOLECULAR LEVEL TRANSFORMATION OF THE SOLID DIFFERENT STATES ➔ Little space between particles ➔ Particles fixed in place but vibrate around a fixed position ➔ Little or no volume change under moderate pressure LIQUID ENDOTHERMIC ➔ Some free space between particles Melting ➔ Particles move past one another Sublimation ➔ Can be compressed lightly by Evaporation moderate pressure EXOTHERMIC GAS Deposition ➔ Particles are widely separated with Freezing much free space Condensation ➔ Particles move through space ➔ Compressed under moderate MELTING (FUSION) - SOLID TO LIQUID pressure ➔ When solid substances such as ice cubes, metals, or wax are supplied with enough amount of heat, they reach their melting point and are changed into liquids. FREEZING - LIQUID TO SOLID ➔ When liquid releases heat, the WATER IN MOLECULAR LEVEL molecules begin to move at a lower pace. The space between the molecules decreases, causing the molecules become compact. Example: Freezing MJT & SMB || 3  LONG TEST 1.1 SCIENCE REVIEWER 9 ___________________________________________________________________ EVAPORATION - LIQUID TO GAS ATOMS ➔ When a liquid absorbs enough ➔ It is the smallest unit of matter heat, it reaches its boiling point that retains its chemical properties. and changes into a gas. Examples: MOLECULES Hot tea getting cold ➔ Atoms can combine to form Boiling water in the kettle (steam) molecules ➔ It is composed of two or more CONDENSATION - GAS TO LIQUID atoms bound together in a discrete ➔ It is the process where water arrangement. vapor becomes liquid. ➔ The atoms bound together in a Examples: molecule can be from the same Water Droplets on the cold drinks element or from different elements Morning drew CLASSIFYING MATTER ACCORDING SUBLIMATION - SOLID TO GAS TO COMPOSITION ➔ It is the process in which a ➔ Have uniform (the same) substance is transformed from chemical composition throughout the solid phase directly to the and from sample to sample gas state without passing the liquid phase. PURE SUBSTANCES Examples: ➔ Made of only one matter; thus, Dry Ice the composition is the same Solid Air Fresheners throughout ➔ Chemical and physical properties DEPOSITION - GAS TO SOLID are constant ➔ It is the opposite of sublimation where Examples: a substance is transformed from Pure Water the gas phase directly to the solid Hydrogen Gas state without passing the liquid phase. Gold Examples: Frost Formation MIXTURE Snowflakes ➔ Made up of several substances that are not chemically bonded T1.4A: Classification of Matter ➔ Chemical and physical properties Based on Composition (PURE may vary SUBSTANCE) Examples: Oil and Water Scanning Tunneling Microscopy (STM) Sugar Solution ➔ a powerful instrument that allows one to image the sample surface PURE SUBSTANCE CAN BE at the atomic level. CLASSIFIED INTO ELEMENTS AND COMPOUNDS ELEMENT ➔ It is composed of only one type of atom. MJT & SMB || 4  LONG TEST 1.1 SCIENCE REVIEWER 9 ___________________________________________________________________ ➔ It is a substance that cannot be spheres of the same size and broken down into simpler color joined together substances even by a chemical reaction. ➔ Chemical symbol identifies an element Examples: Chlorine (CI2) Oxygen (O2) Carbon (C) Phosphorus (P) Copper (Cu) COMPOUND Bromine (Br) ➔ Molecules of compounds are Nickel (Ni) represented by two or more Lead (Pb) spheres of different colors joined Gold (Au) together. Aluminum (Al) Sulfur (S) Tin (Sn) COMPOUND ➔ Composed of two or more elements combined in definite T1.4B: Classification of Matter proportions Based on Composition (MIXTURE) ➔ It can be broken down into smaller compounds, or their basic HOW DOES THE COMPOSITION OF A elements, by chemical change. MIXTURE DIFFER FROM A Examples: SUBSTANCE? Water (H2O) Carbon dioxide (CO2) PURE SUBSTANCES Glucose (C6H12O6) ➔ Have uniform (the same) chemical composition throughout ELEMENTS AND COMPOUND and from sample to sample Sodium (Na) Chlorine gas (CI2) MIXTURE Sodium chloride (NaCI) ➔ Composed of two or more substances and may or may not HOW TO REPRESENT THE have uniform composition PARTICULATE NATURE OF ELEMENTS Examples: AND COMPOUNDS? Lemonade (Mixture of water, lemon juice, sugar) ELEMENT Salad Dressing (Mixture of olive ➔ Atoms of elements are oil, vinegar, herbs, spices) represented by single spheres. ➔ Molecules of elements are represented by two or more MJT & SMB || 5  LONG TEST 1.1 SCIENCE REVIEWER 9 ___________________________________________________________________ MIXTURE DECANTATION ➔ A combination of two or more ➔ It is a process of separating a elements or compounds solid from a liquid, by pouring ➔ Can be separated by physical off the liquid, after allowing the processes. solid to settle in the liquid. Examples: TYPES OF MIXTURE Dirt and Water Oil and Water HETEROGENEOUS Kerosene and Water ➔ Not uniform throughout Milk and Cream ➔ Mechanical Mixture ➔ The mixture is seen FILTRATION Examples: ➔ It is a process of separating a solid Spaghetti from a liquid by pouring the Milk Tea mixture through a porous material such as filter paper. HOMOGENEOUS Examples: ➔ Uniform throughout Ground coffee ➔ Solution Tea Bag ➔ The mixture cannot be seen Examples: EVAPORATION Orange Juice ➔ It is a process in which a liquid is Milk converted to vapor leaving the insoluble solids in the dish. T1.5A: SEPARATING COMPONENTS Examples: OF MIXTURES Hot tea getting cold Boiling water in the kettle SIFTING OR SIEVING ➔ Used to separate a dry mixture SUBLIMATION which contains substances of ➔ It is a process of purifying solids different sizes by passing it by turning into vapor its volatile through a sieve, a device components. containing tiny holes. Examples: Example: Dry ice Sand and Gravel Solid Air fresheners USING MAGNETS SIMPLE DISTILLATION ➔ It is a process which uses magnets ➔ It is a process of separating two to obtain the substances with miscible liquids because of the magnetic properties from a differences in the boiling point. mixture. Examples: Example: Water can be separated in salt Sulfur and Iron Filings solution Distilled Water Concentration of Alcohol MJT & SMB || 6  LONG TEST 1.1 SCIENCE REVIEWER 9 ___________________________________________________________________ FRACTIONAL DISTILLATION ➔ Point D to E = Equilibrium of a ➔ It is a process of separating the Liquid and Gas components of a liquid one by ➔ Point E to F = Gas one while it boils. ➔ A more complex process of distillation. Example: Crude oil CHROMATOGRAPHY ➔ It is a process of separating the component colors of a mixture by dipping a medium into a filter paper soaked in a solvent. Examples: COOLING CURVE Separation of inks, dyes, and ➔ Point A to B = Gas coloring agents ➔ Point B to C = Equilibrium of a Gas and Liquid CENTRIFUGATION ➔ Point C to D = Liquid ➔ It is a technique that, by rotating ➔ Point D to E = Equilibrium of a the sample at high speed, Liquid and Solid separates solids suspended in a ➔ Point E to F = Solid liquid (or liquids of different densities). Examples: Separates red blood cells and white blood cells T1.5B: PHASE CHANGE DIAGRAMS PHASE CHANGE DIAGRAM ➔ A phase change diagram is a graphical representation of the correlation between heat input and the temperature of a substance. PHASE CHANGE DIAGRAM - ➔ It can be used to determine the COMBINED melting point and the boiling point of a substance. HEATING CURVE ➔ Point A to B = Solid ➔ Point B to C = Equilibrium of a Solid and Liquid ➔ Point C to D = Liquid MJT & SMB || 7