Chemical Reactions Notes-1a-1
... Instead, each ion is surrounded by a shell of water molecules. This tends to stabilize the ions in solution and prevent cations and anions from recombining. The positive ions have the surrounding oxygen atoms of water pointing towards the ion, negative ions have the surrounding hydrogen atoms of wat ...
... Instead, each ion is surrounded by a shell of water molecules. This tends to stabilize the ions in solution and prevent cations and anions from recombining. The positive ions have the surrounding oxygen atoms of water pointing towards the ion, negative ions have the surrounding hydrogen atoms of wat ...
makeup2
... freezes at -1.46°C. What is the molecular weight of x? (Kf = 1.86) (A) 84 x 1.86 x 1.46 = 222 g/mol (B) 84 x (1.86 / 1.46) = 107 g/mol (C) 84 x (1.46 / 1.86) = 66 g/mol (D) 1.46 x (1.86 / 84) = 0.032 g/mol 59. A 1.20 liter sample is drawn from a bottle labeled "86.0% by weight H2SO4, density 1.787 g ...
... freezes at -1.46°C. What is the molecular weight of x? (Kf = 1.86) (A) 84 x 1.86 x 1.46 = 222 g/mol (B) 84 x (1.86 / 1.46) = 107 g/mol (C) 84 x (1.46 / 1.86) = 66 g/mol (D) 1.46 x (1.86 / 84) = 0.032 g/mol 59. A 1.20 liter sample is drawn from a bottle labeled "86.0% by weight H2SO4, density 1.787 g ...
IPC – First Semester Exam Review Be able to classify an example
... Potassium (K) is in group 1 and has 1 valence electron. K gives up that 1 electron because it is easier to give up 1 electron than to gain 7 electrons to get a full outer shell. When K gives up the electron, it has one more positive proton than negative electron. Potassium starts with 19 positive pr ...
... Potassium (K) is in group 1 and has 1 valence electron. K gives up that 1 electron because it is easier to give up 1 electron than to gain 7 electrons to get a full outer shell. When K gives up the electron, it has one more positive proton than negative electron. Potassium starts with 19 positive pr ...
Key III
... a) The sigma bond formed between the carbon and oxygen atoms is best described as being between the overlap of a(n) _ __ hybrid orbital on C with a(n) _ __ hybrid orbital on O. b) The sigma bonds formed between the hydrogen and carbon is best described as being the overlap of an __ _ hybrid orbital ...
... a) The sigma bond formed between the carbon and oxygen atoms is best described as being between the overlap of a(n) _ __ hybrid orbital on C with a(n) _ __ hybrid orbital on O. b) The sigma bonds formed between the hydrogen and carbon is best described as being the overlap of an __ _ hybrid orbital ...
ACS Practice Test 1
... (C)an electron pair in the SO2 molecule alternates back and forth between the two sulfur–oxygen electron pairs so that the two different bonds seem to exchange positions. (D)the SO2 molecule revolves so that the two different bonds seem to exchange positions. 58. Which compound would be expected to ...
... (C)an electron pair in the SO2 molecule alternates back and forth between the two sulfur–oxygen electron pairs so that the two different bonds seem to exchange positions. (D)the SO2 molecule revolves so that the two different bonds seem to exchange positions. 58. Which compound would be expected to ...
First Semester complete review with answers
... 33. How do you determine an element’s oxidation number? Use potassium and nitrogen as examples. Oxidation number is determined y how many electrons an atom takes or gives to become an ion. K oxidation number is +1. Potassium (K) is in group 1 and has 1 valence electron. K gives up that 1 electron be ...
... 33. How do you determine an element’s oxidation number? Use potassium and nitrogen as examples. Oxidation number is determined y how many electrons an atom takes or gives to become an ion. K oxidation number is +1. Potassium (K) is in group 1 and has 1 valence electron. K gives up that 1 electron be ...
Practice MSL Multiple Choice 1. Compared to the charge and mass
... The sign of H is positive, and the products have less potential energy than the reactants. The sign of H is positive, and the products have more potential energy than the reactants. The sign of H is negative, and the products have less potential energy than the reactants. The sign of H is negative, ...
... The sign of H is positive, and the products have less potential energy than the reactants. The sign of H is positive, and the products have more potential energy than the reactants. The sign of H is negative, and the products have less potential energy than the reactants. The sign of H is negative, ...
The Mole Ratio · the ratio between the molar amounts of any two
... · the method of predicting the quantity of a reactant or product in a chemical reaction based on the quantity of another reactant or product in the reaction ...
... · the method of predicting the quantity of a reactant or product in a chemical reaction based on the quantity of another reactant or product in the reaction ...
Take notes on this document while you are watching the recorded
... Text Fig. 2.4 p. 31 Hydrogen bond formation in water (BETWEEN WATER MOLECULES) 3. Hydrogen bonds a. Formed between an atom which is partially positively (+) charged and a partially negatively (-) charged atom, especially between a hydrogen (+) atom and a (-) nitrogen, oxygen, or fluorine atom, ofte ...
... Text Fig. 2.4 p. 31 Hydrogen bond formation in water (BETWEEN WATER MOLECULES) 3. Hydrogen bonds a. Formed between an atom which is partially positively (+) charged and a partially negatively (-) charged atom, especially between a hydrogen (+) atom and a (-) nitrogen, oxygen, or fluorine atom, ofte ...
Chemistry Review2
... Note: single replacement reactions only produce products when the single metal in the reactant is more active than the metal in the compound in the reactant. 1.In the equation: Fe + CuSO4 predict products, balance the equation and determine what element is reduced and what element is oxidized. Bal ...
... Note: single replacement reactions only produce products when the single metal in the reactant is more active than the metal in the compound in the reactant. 1.In the equation: Fe + CuSO4 predict products, balance the equation and determine what element is reduced and what element is oxidized. Bal ...
ATOMS, MOLECULES and IONS
... The positive charge (the number of protons) on the nucleus is the Atomic Number of that atom, Z. (This is the number above the element on the Periodic Table.) A sample of any given ELEMENT is comprised of many atoms, all of which have the same atomic number; in Carbon, every atom has 6 e - and a nuc ...
... The positive charge (the number of protons) on the nucleus is the Atomic Number of that atom, Z. (This is the number above the element on the Periodic Table.) A sample of any given ELEMENT is comprised of many atoms, all of which have the same atomic number; in Carbon, every atom has 6 e - and a nuc ...
chemical reaction
... Recall that some elements exist primarily as diatomic molecules, such as H2. Each of these elements is represented in an equation by its molecular formula. Other elements in the elemental state are usually represented simply by their atomic symbols. For Example carbon is represented as C. The symbo ...
... Recall that some elements exist primarily as diatomic molecules, such as H2. Each of these elements is represented in an equation by its molecular formula. Other elements in the elemental state are usually represented simply by their atomic symbols. For Example carbon is represented as C. The symbo ...
Balancing Equations
... When balancing a chemical reaction you may add coefficients in front of the compounds to balance the reaction, but you may not change the subscripts. n Changing the subscripts changes the compound. Subscripts are determined by the valence electrons (charges for ionic or ...
... When balancing a chemical reaction you may add coefficients in front of the compounds to balance the reaction, but you may not change the subscripts. n Changing the subscripts changes the compound. Subscripts are determined by the valence electrons (charges for ionic or ...
Dec. 15 , 2012, 9:00 am – noon - Dr. K. Brown
... 37) A molecule has the formula ML2. Atom M is the central atom and the L-M-L bond angle is 117o. What are the most likely electron groups? A) Two bonds and no non-bonding pairs B) Two bonds and one non-bonding pair C) Two bonds and two non-bonding pairs D) Two bonds and three non-bonding pairs E) T ...
... 37) A molecule has the formula ML2. Atom M is the central atom and the L-M-L bond angle is 117o. What are the most likely electron groups? A) Two bonds and no non-bonding pairs B) Two bonds and one non-bonding pair C) Two bonds and two non-bonding pairs D) Two bonds and three non-bonding pairs E) T ...
Document
... a) The mass of a proton is greater than the mass of an electron. b) A proton is positively charged and an electron is negatively charged. c) Most of the atom’s volume is the sphere-shaped cloud of electrons d) One or more neutrons in the nucleus add mass to the atom. ...
... a) The mass of a proton is greater than the mass of an electron. b) A proton is positively charged and an electron is negatively charged. c) Most of the atom’s volume is the sphere-shaped cloud of electrons d) One or more neutrons in the nucleus add mass to the atom. ...
Physical Science Chapter 7 Chemical Reactions Section 7.1
... Oxidation For a long time, people have known that metals react with oxygen. Calcium reacts with oxygen and forms calcium oxide (CaO). _________________________________ __________________________________________________________________. These types of synthesis _______________________________________ ...
... Oxidation For a long time, people have known that metals react with oxygen. Calcium reacts with oxygen and forms calcium oxide (CaO). _________________________________ __________________________________________________________________. These types of synthesis _______________________________________ ...
Biochemistry-Review of the Basics
... Competitive-wrong substrate in active site Non-competitive- molecule binds to an allosteric site which causes an shape change in the enzyme so the substrate can't bind ...
... Competitive-wrong substrate in active site Non-competitive- molecule binds to an allosteric site which causes an shape change in the enzyme so the substrate can't bind ...
Name
... a. Theoretical yield b. Percentage yield c. Mole ratio d. Actual yield 14. For the reaction Cl2 + 2KBr → 2KCl +Br2, calculate the percentage yield if 200g of chlorine react with excess potassium bromide to produce 410g of bromine. a. 73.4% b. 82.1% c. 91.0% d. 98.9% 15. For the reaction Mg + 2HCl → ...
... a. Theoretical yield b. Percentage yield c. Mole ratio d. Actual yield 14. For the reaction Cl2 + 2KBr → 2KCl +Br2, calculate the percentage yield if 200g of chlorine react with excess potassium bromide to produce 410g of bromine. a. 73.4% b. 82.1% c. 91.0% d. 98.9% 15. For the reaction Mg + 2HCl → ...
Gas and Vapor Phase Explosions
... 4. Heat the platinum gauze in a flame until bright red. Then quickly lower it into the beaker so that it is approximately 1 – 2 centimeters above the surface of the alcohol. The glass rod can be laid across the rim of the beaker. 5. If the alcohol catches fire, smother it by covering the beaker with ...
... 4. Heat the platinum gauze in a flame until bright red. Then quickly lower it into the beaker so that it is approximately 1 – 2 centimeters above the surface of the alcohol. The glass rod can be laid across the rim of the beaker. 5. If the alcohol catches fire, smother it by covering the beaker with ...
chapter 2
... a. Alkali Metals – most reactive metals, react violently with water b. Alkaline Earth Metals – reactive metals but less so than alkali c. Halogens – most reactive non-metals, most are poisonous gases d. Noble Gases – do not react 3. If a noble gas could form a +1 ion, which of the noble gases would ...
... a. Alkali Metals – most reactive metals, react violently with water b. Alkaline Earth Metals – reactive metals but less so than alkali c. Halogens – most reactive non-metals, most are poisonous gases d. Noble Gases – do not react 3. If a noble gas could form a +1 ion, which of the noble gases would ...
Chemical Equations
... Chemical formula A representation of a substance in which the elements are represented by their symbols and subscripts represent the number of atoms of each element ...
... Chemical formula A representation of a substance in which the elements are represented by their symbols and subscripts represent the number of atoms of each element ...
Redox
Redox reactions include all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between species. The term ""redox"" comes from two concepts involved with electron transfer: reduction and oxidation. It can be explained in simple terms: Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.Although oxidation reactions are commonly associated with the formation of oxides from oxygen molecules, these are only specific examples of a more general concept of reactions involving electron transfer.Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid–base reactions. Like acid–base reactions, redox reactions are a matched set, that is, there cannot be an oxidation reaction without a reduction reaction happening simultaneously. The oxidation alone and the reduction alone are each called a half-reaction, because two half-reactions always occur together to form a whole reaction. When writing half-reactions, the gained or lost electrons are typically included explicitly in order that the half-reaction be balanced with respect to electric charge.Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation state — the actual transfer of electrons may never occur. The oxidation state of an atom is the fictitious charge that an atom would have if all bonds between atoms of different elements were 100% ionic. Thus, oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always cause a change in oxidation state, but there are many reactions that are classed as ""redox"" even though no electron transfer occurs (such as those involving covalent bonds).There are simple redox processes, such as the oxidation of carbon to yield carbon dioxide (CO2) or the reduction of carbon by hydrogen to yield methane (CH4), and more complex processes such as the oxidation of glucose (C6H12O6) in the human body through a series of complex electron transfer processes.