Chemistry 1st Semester Mid Term PDF

**GENERAL CHEMISTRY 1** ======================= **Activity 01: The Particulate Nature of Matter** ================================================= - - - - - - - - - - - [THE FOUR MAIN IDEAS IN THE PARTICULATE NATURE OF MATTER:] 1. 2. 3. 4. **Activity 02: Propert...

**GENERAL CHEMISTRY 1** ======================= **Activity 01: The Particulate Nature of Matter** ================================================= - - - - - - - - - - - [THE FOUR MAIN IDEAS IN THE PARTICULATE NATURE OF MATTER:] 1. 2. 3. 4. **Activity 02: Properties of Matter** ===================================== [General Properties of Matter] - characteristics that enable us to **differentiate one material from another**. The fundamental properties that are used to describe matter are the following: a. b. c. d. e. **PHYSICAL PROPERTIES OF MATTER** - - a. b. c. d. e. f. g. **CHEMICAL PROPERTIES OF MATTER** - a. b. c. d. e. Examples: Kerosene Flammability ------------------------------ ---------------------------------------------------------------------------- Wood Combustibility Fossil Fuel Biodegradability Heating Pan Conductivity; 3 types of conductivity: Radiation, Conduction, & Convection Pencil = 0.005 kg Mass Rusted Nail Reactivity Snowfall Freezing Point Boiling water Boiling Point Boiling water at 250 celsius Specific Gravity Boiling water at 2:1 Density **Activity 03: Intensive and Extensive Property of Matter** =========================================================== - - **INTENSIVE PROPERTIES** - - - - - - - - - **EXTENSIVE PROPERTIES** - - - - - - - **CHEMICAL PROPERTIES** - - - - - - - **Activity 05: Pure Substances and Mixtures** ============================================= **Pure/ Chemical Substances-** is composed of **one** type of atom or molecule. - **Mixture-** is composed of **different** types of atoms or molecules that are not **chemically bonded**. - **TYPES OF MIXTURES** a. b. **EXAMPLES:** **HOMOGENEOUS MIXTURE** **HETEROGENEOUS MIXTURE** ------------------------- --------------------------- Alcohol Soda with Ice Gasoline Chocolate chip cookies Steel Oil and water **Activity 06: Methods of Separating Components of Mixture** ============================================================ 1. - - **EXAMPLES:** **EVAPORATION** **RECRYSTALLIZATION** ----------------------------- ------------------------------------ Boiling water and its steam The process of making a rock candy 2. - - 1. 2. - - - - - - **EXAMPLES:** +-----------------------------------+-----------------------------------+ | Purification of Alcohol | **DISTILLATION** | +===================================+===================================+ | Paper Chromatography | **CHROMATOGRAPHY** | +-----------------------------------+-----------------------------------+ | -Coffee/ Tea Filter | **FILTRATION** | | | | | -Chalk and Water | | +-----------------------------------+-----------------------------------+ | Baby oil and Water | **DECANTATION** | +-----------------------------------+-----------------------------------+ | Machine for blood testing | **CENTRIFUGATION** | +-----------------------------------+-----------------------------------+ | \- Sand and Gravel | **SIEVING** | | | | | -Boiled noodles in water | | +-----------------------------------+-----------------------------------+ | Colored clothes from white | **MANUAL PICKING** | | clothes | | +-----------------------------------+-----------------------------------+ | Using magnet to gather all | **USE OF MAGNET** | | metallic | | +-----------------------------------+-----------------------------------+ Activity 08: Errors in Measurement and Significant Figure in Calculations ========================================================================= - 1. 2. - - - - - - - +-----------------------------------+-----------------------------------+ | **KIND OF MEASUREMENT ERROR** | **GIVEN** | +===================================+===================================+ | **Systematic Errors** | - | +-----------------------------------+-----------------------------------+ | **Random Errors** | - | +-----------------------------------+-----------------------------------+ | **Gross Errors** | - | +-----------------------------------+-----------------------------------+ | **Instrumental Errors** | - | +-----------------------------------+-----------------------------------+ | **Observational Errors** | - | +-----------------------------------+-----------------------------------+ | **Environmental Errors** | - | +-----------------------------------+-----------------------------------+ 1. 2. 3. - - 1. 2. 3. 4. 5. +-----------------------------------+-----------------------------------+ | RULE NUMBER OF SIGNIFICANT | GIVEN | | FIGURES | | +===================================+===================================+ | 1 | - - | +-----------------------------------+-----------------------------------+ | 2 | - - | +-----------------------------------+-----------------------------------+ | 3 | - - | +-----------------------------------+-----------------------------------+ | 4 | - - | +-----------------------------------+-----------------------------------+ | 5 | - - | +-----------------------------------+-----------------------------------+ 1. - - - - - - Activity 10: Fundamental Laws of Chemistry ========================================== - - - - **Law of Conservation Mass:** In **June 1783,** **Lavoisier** reacted oxygen with inflammable air, obtaining \"water in a very pure state.\" He concluded that water was not an element but a compound of oxygen and inflammable air, or hydrogen as it is now known. He also decomposed water into oxygen and hydrogen. Both reactions gained the same weight. Lavoisier, explained the phenomenon in his famous textbook, Trait **lmentaire de Chimie**, that \"\... in every operation, **an equal quantity of matter exists both before and after the operation.**\" This concept was also known as the **law of conservation of mass.** - **Law of Constant Composition:** After the discovery of the law of conservation of mass, **Joseph Proust, a french chemist** proposed the **law of constant composition** in the year of **1794.** Proust experiments on metal compounds, metal oxides, carbonates, and sulfides led him to discover another breakthrough in chemistry. He stated that if a **pure compound** is **broken down into its constituent elements**, the masses of the constituents **will always have the same proportions**, regardless of the **quantity or source of the original substance.** **Law of Definite Proportion:** A **chemical compound**, no matter what its **origin or its method of preparation**, always **has the same ratio** by mass of hydrogen to oxygen. Was first enunciated by **joseph proust in 1799** **Law of Multiple Proportion: John Dalton** studied **gasses and gaseous mixtures** under different external conditions. **Building on Proust\'s work**, he noted the **mathematically discrete manner** in which elements combined to **form different compounds.** - +-----------------------------------+-----------------------------------+ | **FUNDAMENTAL LAWS OF CHEMISTRY** | **GIVEN** | +===================================+===================================+ | **Law of Conservation Mass** | - | | | | | | | | | | | | - | +-----------------------------------+-----------------------------------+ | **Law of Constant Motion** | - | +-----------------------------------+-----------------------------------+ | **Law of Definite Proportion** | - | +-----------------------------------+-----------------------------------+ | **Law of Multiple Proportion** | - | +-----------------------------------+-----------------------------------+ (good luck po sa exam!!!- bembem) Created by: Khloe Xyville E. Marcos, Student Congress, Auditor