He had the ability to bring people back to life

Signs of end of the world...

Empty Quran and hafiz will forget the Quran

There will be no food and water

you will forget your name and address

There will be no electricity and gas

Milad 12/9/23 | Quizalize

When Europeans met American Indians in the late 15th century, the people of two continents exchanged many beneficial customs and goods. Europeans received New World crops such as potatoes and corn. American Indians acquired cloth and horses. However, besides the beneficial exchanges, Europeans and American Indians often traded deadly germs–bacteria and viruses–for which they had no immunity. Smallpox and Indians Image 1: Smallpox epidemics helped Europeans conquer the Aztec and Incan Empires of Mexico and South America. North American Indians quickly concluded that contact with Europeans often resulted in devastating diseases that caused widespread death. This drawing, made in the 1500s in Mexico, shows how the disease was passed from a European to an American Indian through simple contact. Many of the diseases that were common in Europe were entirely new to the peoples of North America. Diseases such as tuberculosis and measles could be fatal, but Europeans had developed resistance to the disease, so many people survived. However, when European diseases infected American Indians with no previous exposure, the people suffered terribly. The most devastating of these diseases was smallpox which is caused by a virus (Variola major). Smallpox, like many other diseases, had a latent period of about one week between the time the person was exposed to the disease and the time when signs of the disease became apparent. During this time, the sick person might begin a journey and carry the germs along with him. Anyone the person met would be exposed to smallpox. Anything the victim touched including clothing, bedding, or unwashed dishes carried living germs of smallpox. Cotton Mather Image 2: Cotton Mather was a Boston minister. When smallpox threatened Boston, he remembered reading about how the Turks inoculated people with dried material from smallpox blisters. The inoculation usually gave the person a mild case of the disease and future immunity. The procedure was highly controversial, but it helped save the lives of 274 people who were inoculated during the Boston smallpox epidemic of 1721. Symptoms of the disease began with fever, chills, and aches. The fever might raise a person’s temperature from the normal 98.6o to a dangerous 106o. After four days of misery, the victim entered the second stage when large pustules (fluid-filled bumps) appeared on the body. The rash made the person feel as if their skin were on fire. After suffering with the rash for nine days, the victim entered a new stage-if he or she had survived this long. The pustules opened and dried up. Each pustule formed a scab that turned into a scar that marked the person’s face for the rest of his or her life. Complications of smallpox for those who survived might include loss of vision or damage to the lungs, heart, or liver. Waterhouse Image 3: Dr. Benjamin Waterhouse of Harvard University brought Jenner’s smallpox preventative to the United States. It was called vaccination and used cowpox as the infective material. This much milder form of pox gave immunity to smallpox with fewer complications. Dr. Waterhouse encouraged President-elect Thomas Jefferson to promote vaccination. Jefferson responded, “Every friend of humanity must look with pleasure on this discovery, by which one evil more is withdrawn from the condition of man.” (T. Jefferson 12/25/1800 to Benjamin Waterhouse, December 25, 1800) Historians have found evidence of smallpox as far back as 1157 B.C. when the Egyptian pharaoh Ramses V apparently died of smallpox. From Egypt, where scientists believe smallpox began, the disease spread to Asia. Europeans began to experience periodic epidemics of smallpox in the14th century when Crusaders returning from the Middle East brought smallpox to Europe. People who survived the disease were immune and could not get smallpox again. This fact explains why epidemics struck periodically and the disease was not a constant threat to European societies. Smallpox Vaccination 1803 Image 4: Dr. Edward Jenner’s new smallpox vaccination (from cowpox) was widely accepted. This medical image was published by a Spanish physician to teach colonial doctors how to apply the vaccine to native Mexicans. The scratches were supposed to go through several stages of development as evidence that the vaccine had given the patient immunity. Vaccination was very effective in preventing smallpox epidemics among those who received the vaccine. In 1520, while Cortés was trying to conquer the Aztecs, smallpox broke out among the Spaniards and was transferred to the Aztecs. By 1527, the disease had migrated through Central America to Peru where it helped Pizarro conquer the Incas. (See Image 1.) In 1633, smallpox infected American Indians living near the English colony of Plymouth, Massachusetts. The disease traveled very quickly to tribes living far inland from the English colonies. In 1721, a smallpox epidemic threatened the English colonists of Boston. (See Image 2.) Cotton Mather, a Boston minister, wanted to inoculate people against the disease. He knew that Turkish healers took material from a dried smallpox scab and injected it into the body of a healthy person by scratching the surface of the skin. The patients developed a mild form of the disease from which they recovered. The procedure was highly controversial in Boston where about 280 Bostonians accepted inoculation. The epidemic infected more than half of the people living in Boston at the time. About 15% of those who got sick died of the disease. Among those who were inoculated, only six (2%) died of smallpox. The practice of inoculation spread to other English colonies, but not to the American Indian tribes living near the colonies. Late in the 18th century, British doctor Edward Jenner recognized that people who milked cows never came down with smallpox. They had already been infected with cowpox, a similar, but much milder disease that gave them immunity to smallpox. In 1796, Jenner inoculated a young man with cowpox virus he had collected from a milkmaid. The young man had a mild infection for less than 24 hours and recovered. Jenner’s efforts resulted in a widespread acceptance of vaccination (vaccine comes from Latin words meaning “taken from a cow”). By 1800, many Americans were receiving smallpox vaccinations. (See Image 3.) President Thomas Jefferson supported and encouraged the vaccination program in major American cities. (See Image 4.) By the middle of the 19th century, smallpox was under control, but broke out from time to time among unvaccinated people. Bismarck, Dakota Territory, experienced a small outbreak of smallpox in 1882. American Indians, however, were still subject to the disease in its most dangerous form.

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.

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