MID-TERM EXAM REVIEW! Unit 1 Convert the following: 1.) 2.02 x
... 11.) Potassium iodide completely dissolved in water 12.) Soil 13.) Chromium * Classify as chemical or physical changes. 14.) Shredding cheese 15.) Melting cheese 16.) Digesting cheese 17.) Making salt from sodium and chlorine 18.) Sprinkling salt on french fries * In what group (give number) are eac ...
... 11.) Potassium iodide completely dissolved in water 12.) Soil 13.) Chromium * Classify as chemical or physical changes. 14.) Shredding cheese 15.) Melting cheese 16.) Digesting cheese 17.) Making salt from sodium and chlorine 18.) Sprinkling salt on french fries * In what group (give number) are eac ...
Chemistry Post-Enrolment Worksheet C
... e.g. sodium chloride is made up of Na+ ions and Cl- ions. The overall formula is NaCl lithium oxide is made up of Li+ ions and O2- ions. The overall formula is Li2O Polyatomic ions are those that contain more than one atom e.g. the hydroxide ion (OH -), which is made up of an oxygen atom and a hydro ...
... e.g. sodium chloride is made up of Na+ ions and Cl- ions. The overall formula is NaCl lithium oxide is made up of Li+ ions and O2- ions. The overall formula is Li2O Polyatomic ions are those that contain more than one atom e.g. the hydroxide ion (OH -), which is made up of an oxygen atom and a hydro ...
Chem MCQ for Class-9th
... 2. The amount of energy given out when an electron is added to an atom is called: a. Lattice entery b. ionization entergy c. electronegativity d. electron affinity 3. Mendeleev Periodic Table was based upon the: a. Electronic configuration b. atomic mass c. Atomic number d. completion of subshell 4. ...
... 2. The amount of energy given out when an electron is added to an atom is called: a. Lattice entery b. ionization entergy c. electronegativity d. electron affinity 3. Mendeleev Periodic Table was based upon the: a. Electronic configuration b. atomic mass c. Atomic number d. completion of subshell 4. ...
chemical reaction - Peoria Public Schools
... atoms in nature. These non-metals are found in elemental form as two atoms ...
... atoms in nature. These non-metals are found in elemental form as two atoms ...
Determination of the Atomic Weight of Magnesium CHEM 101
... The accepted value (periodic table) is 24.3 g mol−1 Smith and Jones (2012). The percentage discrepancy between the accepted value and the result obtained here is 1.3%. Because only a single measurement was made, it is not possible to calculate an estimated standard deviation. The most obvious source ...
... The accepted value (periodic table) is 24.3 g mol−1 Smith and Jones (2012). The percentage discrepancy between the accepted value and the result obtained here is 1.3%. Because only a single measurement was made, it is not possible to calculate an estimated standard deviation. The most obvious source ...
Single Replacement Reactions
... Explain the type of reaction that occurred between the acid and metals. Compare and contrast the degree of chemical reactivity among the metals. o How did you decide? Did the lab results support the hypothesis? ...
... Explain the type of reaction that occurred between the acid and metals. Compare and contrast the degree of chemical reactivity among the metals. o How did you decide? Did the lab results support the hypothesis? ...
Chemistry Readings
... An element is a substance made from only one type of atom. For example, Carbon is made entirely from Carbon atoms and Sodium is made entirely from Sodium atoms. An element can not be broken down (chemically) into simpler substance. The Periodic Table shows all known the elements. The Periodic Table ...
... An element is a substance made from only one type of atom. For example, Carbon is made entirely from Carbon atoms and Sodium is made entirely from Sodium atoms. An element can not be broken down (chemically) into simpler substance. The Periodic Table shows all known the elements. The Periodic Table ...
H2, N2, O2, F2, Cl2, Br2, I2
... 3. • Only change the coefficient ( the number in front of the formula ) when balancing. This tells us how many of each molecule or atom we have in the balanced equation. If there is no number in front, a " 1 " is there but we usually leave out the 1's. • Do not change subscripts to balance. They are ...
... 3. • Only change the coefficient ( the number in front of the formula ) when balancing. This tells us how many of each molecule or atom we have in the balanced equation. If there is no number in front, a " 1 " is there but we usually leave out the 1's. • Do not change subscripts to balance. They are ...
Atoms, Molecules and Ions - Moodle @ FCT-UNL
... The rules for naming oxoanions, anions of oxoacids, are as follows: 1. When all the H ions are removed from the “-ic” acid, the anion’s name ends with “-ate.” 2. When all the H ions are removed from the “-ous” acid, the anion’s name ends with “-ite.” 3. The names of anions in which one or more but ...
... The rules for naming oxoanions, anions of oxoacids, are as follows: 1. When all the H ions are removed from the “-ic” acid, the anion’s name ends with “-ate.” 2. When all the H ions are removed from the “-ous” acid, the anion’s name ends with “-ite.” 3. The names of anions in which one or more but ...
Chapter 2 PowerPoint
... The rules for naming oxoanions, anions of oxoacids, are as follows: 1. When all the H ions are removed from the “-ic” acid, the anion’s name ends with “-ate.” 2. When all the H ions are removed from the “-ous” acid, the anion’s name ends with “-ite.” 3. The names of anions in which one or more but n ...
... The rules for naming oxoanions, anions of oxoacids, are as follows: 1. When all the H ions are removed from the “-ic” acid, the anion’s name ends with “-ate.” 2. When all the H ions are removed from the “-ous” acid, the anion’s name ends with “-ite.” 3. The names of anions in which one or more but n ...
Slide 1
... organic groups (aliphatic or aromatic or a mixture of both). There are three classes of amines. ...
... organic groups (aliphatic or aromatic or a mixture of both). There are three classes of amines. ...
Notebook - Science
... carbon: found free in the form of diamond and graphite, is a component of natural gas, petroleum, and coal, combines with oxygen to form carbon dioxide and carbonate in limestone and chalk, forms carbides, cyanides, and oxides nitrogen: 78% of air by volume, essential element of life, a component of ...
... carbon: found free in the form of diamond and graphite, is a component of natural gas, petroleum, and coal, combines with oxygen to form carbon dioxide and carbonate in limestone and chalk, forms carbides, cyanides, and oxides nitrogen: 78% of air by volume, essential element of life, a component of ...
Section 2 Types of Chemical Reactions Chapter 8
... CH4(g) + O2(g) CO2(g) + 2H2O(g) (partially balanced) • Now consider the number of oxygen atoms. • Increase the number of oxygen atoms on the left side to four by placing the coefficient 2 in front of the molecular formula ...
... CH4(g) + O2(g) CO2(g) + 2H2O(g) (partially balanced) • Now consider the number of oxygen atoms. • Increase the number of oxygen atoms on the left side to four by placing the coefficient 2 in front of the molecular formula ...
Chemistry
... states of matter and changes between the physical states of matter. 2. Determine rates of chemical reactions and the variables that affect chemical reaction rates. 3. Assess experimental data for mechanistic features of a chemical reaction. 4. Identify the constituents of a system at chemical equili ...
... states of matter and changes between the physical states of matter. 2. Determine rates of chemical reactions and the variables that affect chemical reaction rates. 3. Assess experimental data for mechanistic features of a chemical reaction. 4. Identify the constituents of a system at chemical equili ...
Unit 1 Powerpoint
... B2.5A Recognize and explain that macromolecules such as lipids contain high energy bonds. B2.2B - Recognize the six most common elements in organic molecules (C, H, N, O, P, S). B2.2A - Explain how carbon can join to other carbon atoms in chains and rings to form large and complex molecules. B2.2C - ...
... B2.5A Recognize and explain that macromolecules such as lipids contain high energy bonds. B2.2B - Recognize the six most common elements in organic molecules (C, H, N, O, P, S). B2.2A - Explain how carbon can join to other carbon atoms in chains and rings to form large and complex molecules. B2.2C - ...
I. scientific notation. – a shorthand that scientists use when dealing
... a. Temperature – the intensity of heat in a body, that is, how hot or how cold the body is. Three different temperature scales represent same temp: i.Fahrenheit – bp H2O 212ºF ii.Celsius – bp H2O 100ºC 5 x (ºF – 32)/9 iii.Kelvin - bp H2O 373 K (Celsius + 273) b. the SI unit of heat and energy is the ...
... a. Temperature – the intensity of heat in a body, that is, how hot or how cold the body is. Three different temperature scales represent same temp: i.Fahrenheit – bp H2O 212ºF ii.Celsius – bp H2O 100ºC 5 x (ºF – 32)/9 iii.Kelvin - bp H2O 373 K (Celsius + 273) b. the SI unit of heat and energy is the ...
SG5 Chemical Reactions and Quantities
... A student who completes this unit should be able to do all of the following: 1) Define a chemical reaction A rearrangement of atoms in which compounds may break down and new compounds may form 2) Identify evidence for a chemical reaction Heat is either consumed (endothermic process) or released (exo ...
... A student who completes this unit should be able to do all of the following: 1) Define a chemical reaction A rearrangement of atoms in which compounds may break down and new compounds may form 2) Identify evidence for a chemical reaction Heat is either consumed (endothermic process) or released (exo ...
Matter - HCC Learning Web
... • All substances have kinetic energy no matter what physical state they are in. • Solids have the lowest kinetic energy, and gases have the greatest kinetic energy. • As you increase the temperature of a substance, its kinetic energy increases. ...
... • All substances have kinetic energy no matter what physical state they are in. • Solids have the lowest kinetic energy, and gases have the greatest kinetic energy. • As you increase the temperature of a substance, its kinetic energy increases. ...
ch14
... The large number and wide variety of organic compounds is due to the ability of C to bond to itself, and to form multiple bonds. Catenation is the process whereby carbon bonds to itself to form stable chains, branches, and rings. Since C is small, the C-C bond is short enough to allow effective side ...
... The large number and wide variety of organic compounds is due to the ability of C to bond to itself, and to form multiple bonds. Catenation is the process whereby carbon bonds to itself to form stable chains, branches, and rings. Since C is small, the C-C bond is short enough to allow effective side ...
History of chemistry
The history of chemistry represents a time span from ancient history to the present. By 1000 BC, civilizations used technologies that would eventually form the basis to the various branches of chemistry. Examples include extracting metals from ores, making pottery and glazes, fermenting beer and wine, extracting chemicals from plants for medicine and perfume, rendering fat into soap, making glass, and making alloys like bronze.The protoscience of chemistry, alchemy, was unsuccessful in explaining the nature of matter and its transformations. However, by performing experiments and recording the results, alchemists set the stage for modern chemistry. The distinction began to emerge when a clear differentiation was made between chemistry and alchemy by Robert Boyle in his work The Sceptical Chymist (1661). While both alchemy and chemistry are concerned with matter and its transformations, chemists are seen as applying scientific method to their work.Chemistry is considered to have become an established science with the work of Antoine Lavoisier, who developed a law of conservation of mass that demanded careful measurement and quantitative observations of chemical phenomena. The history of chemistry is intertwined with the history of thermodynamics, especially through the work of Willard Gibbs.