Adding g to kg, ml to L

4. Food Storage Methods Food storage means keeping food safely for future use. 🌍 A. Indigenous (Traditional) Storage Methods 4 These are methods used long ago and still used in rural areas: Drying (Sun drying) – removing water from food (e.g. vegetables, meat) Smoking – preserving meat or fish using smoke Salting – adding salt to prevent spoilage Fermentation – changing food using microorganisms (e.g. sour milk) Use of granaries – storing grains in raised structures Clay pots – keeping food cool and fresh 🧊 B. Modern Storage Methods 6 These use technology to keep food fresh: Refrigeration – keeping food cold in a fridge Freezing – storing food at very low temperatures Canning – sealing food in tins Bottling – storing liquids in sealed bottles Vacuum sealing – removing air from packaging Use of preservatives – adding chemicals to prevent spoilage ⭐ 5. Importance of Food Storage Prevents food from going bad Reduces food wastage Saves money Ensures food is available in times of shortage Maintains food quality and safety

1. Settlements Importance of Rivers Fertile Land: The soil near rivers was great for farming, thanks to regular flooding that added nutrients. Trade and Travel: Rivers made moving things and people easy, which helped trade and communication. Protection: Rivers could act as natural barriers, making it harder for enemies to attack. Food: Rivers were full of fish and other food, adding to what people could eat. Energy: People used the river's flow to power machines, for example, grinding grain. Cleanliness: Rivers were used to wash away waste, keeping settlements cleaner. Culture: Rivers often had spiritual importance, and ceremonies and stories revolved around them. Common Geographic Features of Ancient Civilizations Mesopotamia: the Tigris and Euphrates Rivers in central Iraq Indus River Valley: the river runs in the northwestern part of India Nile River Valley: the major river of Egypt Yellow River Valley: a major river flowing through the southern part of China Rivers provided water, food, transportation, and shaped the way of life and development of these ancient civilizations. Impact of Mountains on Settlements Mountains served as barriers to early settlement due to the lack of technology to cross them. The Himalayan Mountains isolated much of India and China during their early development. Impact of Deserts on Migration Deserts posed significant challenges to people who wanted to migrate due to their harsh and unforgiving conditions. Notable deserts include the Empty Quarter in Saudi Arabia and the Sahara Desert in Africa. Changes in Migration and Cultural Blending Advancements in transportation technology post-Industrial Revolution increased cultural blending. Transportation advancements enabled global migration. Before, cultures were isolated, focusing on beliefs and local adaptations. The Industrial Revolution transformed migration and cultural blending. 2. How Humans Modify and Adapt to Their Environment Ways Humans Modify Their Environment Mining: Removing the earth's surface for precious metals. Irrigation: Diverting water for farming. Transportation: Moving goods with trains, cars, airplanes, and boats. Mining Strip mining removes large layers of the earth. Can impact the environment by removing plants and polluting water sources. Irrigation Diverting water for farming and urban development. Transportation Moving goods using trains, cars, airplanes, and boats. Human Adaptation to the Environment Adjusting to environmental conditions by changing behavior. Examples: Wearing specific clothing, using specific building materials. Human Modification of the Environment Changing the earth to meet human needs by physically altering the environment. Examples: Dams, canals, roads, bridges. Impact of Weather and Geological Events on Humans Events like earthquakes, hurricanes, and cold weather affect human settlements. Examples: Building earthquake-resistant buildings, creating levees, using ice for tourism. 3. Understanding Culture Introduction to Culture Culture refers to the way of life of a group of people who live in a particular place. It includes traditions, beliefs, values, and the way they do things. Cultural Characteristics Religious traditions Language Family values Laws Cultural characteristics make each culture unique. Cultural Representations Art Architecture Music Literature Cultural representations express a culture's creativity and show their beliefs and history to the world. Government and Culture Types of government reflect cultural beliefs and traditions. Examples: democratic republic, communist state. The way a country is governed tells a lot about its culture. Economic Systems and Cultures Economic systems reflect cultural values. Examples: bartering, modern economies (e.g., United States, China). How people earn and spend money also reflects their culture. Spread of Cultural Ideas Trade: Spreading ideas through interactions during trade. Travel: Visitors bringing new ideas. War: Conquering armies imposing beliefs. Cultural ideas spread through trade, travel, and war. Multicultural Societies Blending of multiple cultural and ethnic groups. Common in advanced societies with immigration. Multicultural societies create something new by bringing together different cultures. Cultural Adaptation Cultures can change and adapt by taking new ideas and blending them with their own traditions. Example: 'Tex-Mex' food, which blends Mexican and Texan traditions.

Covalent Molecules and Compounds Just as an atom is the simplest unit that has the fundamental chemical properties of an element, a molecule is the simplest unit that has the fundamental chemical properties of a covalent compound. Some pure elements exist as covalent molecules. Hydrogen, nitrogen, oxygen, and the halogens occur naturally as the diatomic (“two atoms”) molecules H2, N2, O2, F2, Cl2, Br2, and I2 (part (a) in Figure 3.1.1). Similarly, a few pure elements exist as polyatomic (“many atoms”) molecules, such as elemental phosphorus and sulfur, which occur as P4 and S8 (part (b) in Figure 3.1.1). Each covalent compound is represented by a molecular formula, which gives the atomic symbol for each component element, in a prescribed order, accompanied by a subscript indicating the number of atoms of that element in the molecule. The subscript is written only if the number of atoms is greater than 1. For example, water, with two hydrogen atoms and one oxygen atom per molecule, is written as H2O. Similarly, carbon dioxide, which contains one carbon atom and two oxygen atoms in each molecule, is written as CO2. Covalent compounds that predominantly contain carbon and hydrogen are called organic compounds. The convention for representing the formulas of organic compounds is to write carbon first, followed by hydrogen and then any other elements in alphabetical order (e.g., CH4O is methyl alcohol, a fuel). Compounds that consist primarily of elements other than carbon and hydrogen are called inorganic compounds; they include both covalent and ionic compounds. In inorganic compounds, the component elements are listed beginning with the one farthest to the left in the periodic table, as in CO2 or SF6. Those in the same group are listed beginning with the lower element and working up, as in ClF. By convention, however, when an inorganic compound contains both hydrogen and an element from groups 13–15, hydrogen is usually listed last in the formula. Examples are ammonia (NH3) and silane (SiH4). Compounds such as water, whose compositions were established long before this convention was adopted, are always written with hydrogen first: Water is always written as H2O, not OH2. The conventions for inorganic acids, such as hydrochloric acid (HCl) and sulfuric acid (H2SO4), are described elswhere. Note! For organic compounds: write C first, then H, and then the other elements in alphabetical order. For molecular inorganic compounds: start with the element at far left in the periodic table; list elements in same group beginning with the lower element and working up. Write the molecular formula of each compound. a. The phosphorus-sulfur compound that is responsible for the ignition of so-called strike anywhere matches has 4 phosphorus atoms and 3 sulfur atoms per molecule. b. Ethyl alcohol, the alcohol of alcoholic beverages, has 1 oxygen atom, 2 carbon atoms, and 6 hydrogen atoms per molecule. c. Freon-11, once widely used in automobile air conditioners and implicated in damage to the ozone layer, has 1 carbon atom, 3 chlorine atoms, and 1 fluorine atom per molecule. Solution: a. • A The molecule has 4 phosphorus atoms and 3 sulfur atoms. Because the compound does not contain mostly carbon and hydrogen, it is inorganic. • B Phosphorus is in group 15, and sulfur is in group 16. Because phosphorus is to the left of sulfur, it is written first. • C Writing the number of each kind of atom as a right-hand subscript gives P4S3 as the molecular formula. b. • A Ethyl alcohol contains predominantly carbon and hydrogen, so it is an organic compound. • B The formula for an organic compound is written with the number of carbon atoms first, the number of hydrogen atoms next, and the other atoms in alphabetical order: CHO. • C Adding subscripts gives the molecular formula C2H6O. c. • A Freon-11 contains carbon, chlorine, and fluorine. It can be viewed as either an inorganic compound or an organic compound (in which fluorine has replaced hydrogen). The formula for Freon-11 can therefore be written using either of the two conventions. • B According to the convention for inorganic compounds, carbon is written first because it is farther left in the periodic table. Fluorine and chlorine are in the same group, so they are listed beginning with the lower element and working up: CClF. Adding subscripts gives the molecular formula CCl3F. • C We obtain the same formula for Freon-11 using the convention for organic compounds. The number of carbon atoms is written first, followed by the number of hydrogen atoms (zero) and then the other elements in alphabetical order, also giving CCl3F. Write the molecular formula for each compound. a. Nitrous oxide, also called “laughing gas,” has 2 nitrogen atoms and 1 oxygen atom per molecule. Nitrous oxide is used as a mild anesthetic for minor surgery and as the propellant in cans of whipped cream. b. Sucrose, also known as cane sugar, has 12 carbon atoms, 11 oxygen atoms, and 22 hydrogen atoms. c. Sulfur hexafluoride, a gas used to pressurize “unpressurized” tennis balls and as a coolant in nuclear reactors, has 6 fluorine atoms and 1 sulfur atom per molecule. Answer: a. N2O b. C12H22O11 c. SF6. Ionic Compounds The substances described in the preceding discussion are composed of molecules that are electrically neutral; that is, the number of positively-charged protons in the nucleus is equal to the number of negatively-charged electrons. In contrast, ions are atoms or assemblies of atoms that have a net electrical charge. Ions that contain fewer electrons than protons have a net positive charge and are called cations. Conversely, ions that contain more electrons than protons have a net negative charge and are called anions. Ionic compounds contain both cations and anions in a ratio that results in no net electrical charge. Note! Ionic compounds contain both cations and anions in a ratio that results in zero electrical charge.An ionic compound that contains only two elements, one present as a cation and one as an anion, is called a binary ionic compound. One example is MgCl2, a coagulant used in the preparation of tofu from soybeans. For binary ionic compounds, the subscripts in the empirical formula can also be obtained by crossing charges: use the absolute value of the charge on one ion as the subscript for the other ion. This method is shown schematically as follows: Crossing charges. One method for obtaining subscripts in the empirical formula is by crossing charges. When crossing charges, it is sometimes necessary to reduce the subscripts to their simplest ratio to write the empirical formula. Consider, for example, the compound formed by Mg2+ and O2−. Using the absolute values of the charges on the ions as subscripts gives the formula Mg2O2:Polyatomic Ions Polyatomic ions are groups of atoms that bear net electrical charges, although the atoms in a polyatomic ion are held together by the same covalent bonds that hold atoms together in molecules. Just as there are many more kinds of molecules than simple elements, there are many more kinds of polyatomic ions than monatomic ions. Two examples of polyatomic cations are the ammonium (NH4+) and the methylammonium (CH3NH3+) ions. P. The method used to predict the empirical formulas for ionic compounds that contain monatomic ions can also be used for compounds that contain polyatomic ions. The overall charge on the cations must balance the overall charge on the anions in the formula unit. Thus, K+ and NO3− ions combine in a 1:1 ratio to form KNO3 (potassium nitrate or saltpeter), a major ingredient in black gunpowder. Similarly, Ca2+ and SO42− form CaSO4 (calcium sulfate), which combines with varying amounts of water to form gypsum and plaster of Paris. The polyatomic ions NH4+ and NO3− form NH4NO3 (ammonium nitrate), a widely used fertilizer and, in the wrong hands, an explosive. One example of a compound in which the ions have charges of different magnitudes is calcium phosphate, which is composed of Ca2+ and PO43− ions; it is a major component of bones. The compound is electrically neutral because the ions combine in a ratio of three Ca2+ ions [3(+2) = +6] for every two ions [2(−3) = −6], giving an empirical formula of Ca3(PO4)2; the parentheses around PO4 in the empirical formula indicate that it is a polyatomic ion. Writing the formula for calcium phosphate as Ca3P2O8 gives the correct number of each atom in the formula unit, but it obscures the fact that the compound contains readily identifiable PO43− ions.Summary • There are two fundamentally different kinds of chemical bonds (covalent and ionic) that cause substances to have very different properties. • The composition of a compound is represented by an empirical or molecular formula, each consisting of at least one formula unit.Contributors The atoms in chemical compounds are held together by attractive electrostatic interactions known as chemical bonds. Ionic compounds contain positively and negatively charged ions in a ratio that results in an overall charge of zero. The ions are held together in a regular spatial arrangement by electrostatic forces. Most covalent compounds consist of molecules, groups of atoms in which one or more pairs of electrons are shared by at least two atoms to form a covalent bond. The atoms in molecules are held together by the electrostatic attraction between the positively charged nuclei of the bonded atoms and the negatively charged electrons shared by the nuclei. The molecular formula of a covalent compound gives the types and numbers of atoms present. Compounds that contain predominantly carbon and hydrogen are called organic compounds, whereas compounds that consist primarily of elements other than carbon and hydrogen are inorganic compounds. Diatomic molecules contain two atoms, and polyatomic molecules contain more than two. A structural formula indicates the composition and approximate structure and shape of a molecule. Single bonds, double bonds, and triple bonds are covalent bonds in which one, two, and three pairs of electrons, respectively, are shared between two bonded atoms. Atoms or groups of atoms that possess a net electrical charge are called ions; they can have either a positive charge (cations) or a negative charge (anions). Ions can consist of one atom (monatomic ions) or several (polyatomic ions). The charges on monatomic ions of most main group elements can be predicted from the location of the element in the periodic table. Ionic compounds usually form hard crystalline solids with high melting points. Covalent molecular compounds, in contrast, consist of discrete molecules held together by weak intermolecular forces and can be gases, liquids, or solids at room temperature and pressure. An empirical formula gives the relative numbers of atoms of the elements in a compound, reduced to the lowest whole numbers. The formula unit is the absolute grouping represented by the empirical formula of a compound, either ionic or covalent. Empirical formulas are particularly useful for describing the composition of ionic compounds, which do not contain readily identifiable molecules. Some ionic compounds occur as hydrates, which contain specific ratios of loosely bound water molecules called waters of hydration.

Identifying rational algebraic expressions vs. non-rational expressions Determining when a rational expression is undefined Naming parts of a rational expression (numerator and denominator) Finding the domain and restrictions Simplifying rational expressions through factoring and cancellation Adding, subtracting, multiplying, and dividing rational expressions Common errors (e.g., incorrect cancellation) Problem-solving with rational expressions

Adding Dissimilar Fractions

Adding 2 numbers under 50

adding

Related quizzes

Related quizzes