Alkanes and isomers
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This document provides information about saturated hydrocarbons including their general formula of CnH2n+2 and lists examples from methane to decane. It asks which molecule is the straight chain form of butane and which is the branched-chain form, noting that isomers have the same molecular formula but different arrangements of atoms.
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Alkanes
The document discusses alkanes, which are hydrocarbons made of carbon and hydrogen. Alkanes form covalent bonds and their structures include methane, ethane, propane, butane, and pentane. The physical states of alkanes depend on the number of carbon atoms, with those under 4 being gases, 4-17 being liquids, and over 17 being solids. Alkanes burn but do not react with acids or alkalis due to the strength of their carbon-carbon single bonds.
Hydrocarbon
Carbon atoms have unique properties that allow them to form long chains and a variety of compounds. Specifically, carbon atoms can form 4 covalent bonds, enabling them to bond to other carbon atoms. This gives carbon the ability to form extensive hydrocarbon chains and complex carbon-based molecules like polymers. Hydrocarbons are compounds composed of only carbon and hydrogen, while carboxides contain carbon and oxygen. Within carbon chains, atoms can occupy primary, secondary, tertiary, or quarternary positions depending on how many other carbon atoms they are bonded to.
Combustion of hydrocarbon
1. Hydrocarbons are organic compounds made of only carbon and hydrogen. They can be classified as saturated or unsaturated depending on the bonding between carbon atoms.
2. Saturated hydrocarbons contain only single bonds between carbons, like alkanes. Unsaturated hydrocarbons contain at least one double bond between carbons, like alkenes.
3. Hydrocarbons undergo complete or incomplete combustion with oxygen, producing carbon dioxide, water, and sometimes carbon monoxide or soot depending on the availability of oxygen.
7.1 tetrahedral carbon alkanes 7.1 (1)
The document discusses alkanes, a class of saturated hydrocarbons with the general formula CnH2n+2. It provides examples of common alkanes like methane, ethane, propane and butane. The document notes that alkanes have single bonds, tetrahedral molecular geometry, and physical properties like being gases at low molecular weights and liquids at higher weights, insoluble in water but soluble in non-polar solvents. It concludes that alkanes are used as fuels in mixtures like petrol, diesel, LPG and natural gas.
Carbon
1. The document is a science lesson about carbon that discusses its occurrence, bonding properties, and ability to form large numbers of compounds.
2. It explains that carbon forms covalent bonds by sharing electrons and can share 1, 2, or 3 pairs of electrons to form single, double, or triple bonds.
3. The document also discusses functional groups, homologous series of hydrocarbons including alkanes, alkenes and alkynes, and isomerism among carbon compounds.
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The document discusses the periodic table, including its development by Mendeleev in 1869 and key elements and groups within it. It notes that Group 1 elements like lithium, sodium, and potassium are alkali metals, while Group 7 elements have increasing atomic numbers and are acidic. The modern periodic table orders elements by increasing atomic number and notes properties of Groups 0, 1, 2, and noble gases.
Naming covalentcompounds
This document provides instructions on naming and writing formulas for binary covalent compounds. It lists Greek prefixes used to denote the number of atoms and gives rules for naming compounds from their formulas and writing formulas from compound names. Examples are given to demonstrate both naming compounds and writing formulas. Practice problems with answers are included to allow applying the rules.
Ch 05 molecules and compounds
This document outlines key concepts about molecules and compounds including:
1) Compounds have constant compositions with the same proportions of elements. Formulas represent atoms in molecules with subscripts.
2) Elements exist as single atoms or diatomic/polyatomic molecules. Molecular compounds form between nonmetals, while ionic compounds form between metals and nonmetals.
3) Formulas for ionic compounds contain positive and negative ions to be electrically neutral. Naming involves the cation name and anion name or polyatomic ion name.
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Alkanes
The document discusses alkanes, which are hydrocarbons made of carbon and hydrogen. Alkanes form covalent bonds and their structures include methane, ethane, propane, butane, and pentane. The physical states of alkanes depend on the number of carbon atoms, with those under 4 being gases, 4-17 being liquids, and over 17 being solids. Alkanes burn but do not react with acids or alkalis due to the strength of their carbon-carbon single bonds.
Hydrocarbon
Carbon atoms have unique properties that allow them to form long chains and a variety of compounds. Specifically, carbon atoms can form 4 covalent bonds, enabling them to bond to other carbon atoms. This gives carbon the ability to form extensive hydrocarbon chains and complex carbon-based molecules like polymers. Hydrocarbons are compounds composed of only carbon and hydrogen, while carboxides contain carbon and oxygen. Within carbon chains, atoms can occupy primary, secondary, tertiary, or quarternary positions depending on how many other carbon atoms they are bonded to.
Combustion of hydrocarbon
1. Hydrocarbons are organic compounds made of only carbon and hydrogen. They can be classified as saturated or unsaturated depending on the bonding between carbon atoms.
2. Saturated hydrocarbons contain only single bonds between carbons, like alkanes. Unsaturated hydrocarbons contain at least one double bond between carbons, like alkenes.
3. Hydrocarbons undergo complete or incomplete combustion with oxygen, producing carbon dioxide, water, and sometimes carbon monoxide or soot depending on the availability of oxygen.
7.1 tetrahedral carbon alkanes 7.1 (1)
The document discusses alkanes, a class of saturated hydrocarbons with the general formula CnH2n+2. It provides examples of common alkanes like methane, ethane, propane and butane. The document notes that alkanes have single bonds, tetrahedral molecular geometry, and physical properties like being gases at low molecular weights and liquids at higher weights, insoluble in water but soluble in non-polar solvents. It concludes that alkanes are used as fuels in mixtures like petrol, diesel, LPG and natural gas.
Carbon
1. The document is a science lesson about carbon that discusses its occurrence, bonding properties, and ability to form large numbers of compounds.
2. It explains that carbon forms covalent bonds by sharing electrons and can share 1, 2, or 3 pairs of electrons to form single, double, or triple bonds.
3. The document also discusses functional groups, homologous series of hydrocarbons including alkanes, alkenes and alkynes, and isomerism among carbon compounds.
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The document discusses the periodic table, including its development by Mendeleev in 1869 and key elements and groups within it. It notes that Group 1 elements like lithium, sodium, and potassium are alkali metals, while Group 7 elements have increasing atomic numbers and are acidic. The modern periodic table orders elements by increasing atomic number and notes properties of Groups 0, 1, 2, and noble gases.
Naming covalentcompounds
This document provides instructions on naming and writing formulas for binary covalent compounds. It lists Greek prefixes used to denote the number of atoms and gives rules for naming compounds from their formulas and writing formulas from compound names. Examples are given to demonstrate both naming compounds and writing formulas. Practice problems with answers are included to allow applying the rules.
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Acids & bases
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Major molecule properties
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Density is a measurement of how much mass is contained within a given volume, calculated by dividing the mass of an object by its volume. A document provides instructions on how to calculate the density of a substance with a mass of 17.63g and volume of 43cm3, which equals 0.41 g/cm3, identifying the substance as the least dense of those listed.
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This document discusses different units for expressing concentration of solutions, including percent, parts per hundred (pph), and parts per million (ppm). It provides an example of calculating the concentration in percent by mass of a solution containing 25 g of sucrose dissolved in 175 g of water.
Digestion acids
Acids have a pH between 1 and 7, with stronger acids having a lower pH. They are able to break down chemicals into smaller parts through chemical reactions. Our bodies use acid in digestion to break down food. Hydrochloric acid in the stomach has a very low pH of 2.0 and helps break down food, though the stomach is lined with mucus to protect it from this strong acid. Heartburn occurs when stomach acid rises into the esophagus, and is often treated by neutralizing the acid with products containing calcium carbonate like TUMS.
Acids & bases
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Covalent bonding
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Solubility
Something dissolved in the Snake River could have caused the fish kill. Polar molecules and ionic compounds can dissolve in water due to the attractions between the water molecules and these substances. The rule is that "like dissolves like," so polar substances dissolve in polar water, while nonpolar substances do not. As temperature increases, the solubility of solids and gases generally increases and decreases, respectively, as shown by solubility curves.
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This document discusses the physical and chemical properties of matter. It defines matter as anything that has mass and takes up space. Physical properties can be observed without changing the material and include characteristics like color, hardness, and melting point. Chemical properties involve a change in the material's composition through reactions with other substances, such as rusting or burning. Some examples provided assess whether various phenomena are physical or chemical properties.
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Density
Density is a measurement of how much mass is contained within a given volume, calculated by dividing the mass of an object by its volume. A document provides instructions on how to calculate the density of a substance with a mass of 17.63g and volume of 43cm3, which equals 0.41 g/cm3, identifying the substance as the least dense compared to others.
Density
Density is a measurement of how much mass is contained within a given volume, calculated by dividing the mass of an object by its volume. A document provides instructions on how to calculate the density of a substance with a mass of 17.63g and volume of 43cm3, which equals 0.41 g/cm3, identifying the substance as the least dense of those listed.
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Pressure & Volume
This document discusses the kinetic molecular theory and Boyle's law. It explains that gases are made of molecules that are far apart from each other and move randomly, colliding with the container walls. According to Boyle's law, if the volume of a container decreases, the pressure increases because the molecules collide with the walls more frequently. The document provides the formula for Boyle's law, P1V1 = P2V2, and gives examples of using it to calculate pressure and volume.
Pressure
Pressure is defined as force per unit area. It can be measured in units such as pounds per square inch, atmospheres, or pascals. Air pressure in the atmosphere is caused by gas molecules constantly colliding with surfaces and exerting force. Standard air pressure at sea level is approximately 101 kPa or 14.7 psi. Pressure calculations involve dividing the total force by the area over which that force is applied.
Matter notes
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Volume notes
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Alkanes and isomers
- 2. Remember: 1) saturated- all single covalent bonds and carbon bonded to 4 atoms 2) CnH2n+2
- 3. # of Name Molecular Carbons Formula 1. METHANE CH4 2. ETHANE C2H6 3. PROPANE C3H8 4. BUTANE C4H10 5. PENTANE C5H12 6. HEXANE C6H14 7. HEPTANE C7H16 8. OCTANE C8H18 9. NONANE C9H20 10. DECANE C10H22
- 4. All carbons in a row Which is the straight chain form of butane?
- 5. All the carbons are not in a row. Which is the branched-chain for of butane?
- 6. Molecules with the same molecular formulas but different arrangement of atoms. Must have at least 4 carbons