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chemia simr01 en - Leszek Niedzicki
... obtaining fully occupied outermost electron subshell. Depending on the starting point - in which direction the target is closer - they can ‘accept’ (acceptor) electrons from other atoms or ‘donate’ (donor) electrons to the bond (share them). • Additionally, bonding is also beneficial energetically – ...
... obtaining fully occupied outermost electron subshell. Depending on the starting point - in which direction the target is closer - they can ‘accept’ (acceptor) electrons from other atoms or ‘donate’ (donor) electrons to the bond (share them). • Additionally, bonding is also beneficial energetically – ...
chapter 5 - chemical reactions
... 1. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) 2. H2SO4(aq) + 2 KOH(aq) K2SO4(aq) + 2 H2O(l) 3. HC2H3O2(aq) + NaOH(aq) NaC2H3O2(aq) + H2O(l) Some double-displacement reactions may result in both the formation of precipitates and water. They can be classified as both precipitation and acid-base reacti ...
... 1. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) 2. H2SO4(aq) + 2 KOH(aq) K2SO4(aq) + 2 H2O(l) 3. HC2H3O2(aq) + NaOH(aq) NaC2H3O2(aq) + H2O(l) Some double-displacement reactions may result in both the formation of precipitates and water. They can be classified as both precipitation and acid-base reacti ...
Chapter 4 Notes
... Example: in NaH, the H is H-; in HCl, the H is H+. + + 2. The oxidation number of a free element is always 0. Example: The atoms in He and N2, for example, have oxidation numbers of 0. 3. The oxidation number of a monatomic ion equals the charge of the ion. Example: oxidation number of Na+ is +1; th ...
... Example: in NaH, the H is H-; in HCl, the H is H+. + + 2. The oxidation number of a free element is always 0. Example: The atoms in He and N2, for example, have oxidation numbers of 0. 3. The oxidation number of a monatomic ion equals the charge of the ion. Example: oxidation number of Na+ is +1; th ...
1. Select the correct statement about subatomic particles. a
... 93. When two substances react to form products, the reactant, which is used up is called the _______. a. determining reagent d. catalytic reagent b. limiting reagent e. reactive reagent c. excess reagent 94. When an equation is used to calculate the amount of product that will form during a reaction ...
... 93. When two substances react to form products, the reactant, which is used up is called the _______. a. determining reagent d. catalytic reagent b. limiting reagent e. reactive reagent c. excess reagent 94. When an equation is used to calculate the amount of product that will form during a reaction ...
Document
... Atoms with 2-3 valence electrons will LOSE electrons and become more positive. Who will lose and who will gain an electron? ...
... Atoms with 2-3 valence electrons will LOSE electrons and become more positive. Who will lose and who will gain an electron? ...
CHEMISTRY 3
... forcing the same equilibrium to shift itself in the reverse direction, ie to the left. (a) ...
... forcing the same equilibrium to shift itself in the reverse direction, ie to the left. (a) ...
Name: Midterm Review (Part II) Fill in the blanks (Chapter 6.1 – 6.3
... Fill in the blanks (Chapter 6.1 – 6.3): In the periodic table, each row is called a _______________________________ . Each column in the periodic table is called a ______________________ . The elements in each period have the same number of_______________________. Each of the elements in the same gr ...
... Fill in the blanks (Chapter 6.1 – 6.3): In the periodic table, each row is called a _______________________________ . Each column in the periodic table is called a ______________________ . The elements in each period have the same number of_______________________. Each of the elements in the same gr ...
UNIT 1 - StudyGuide.PK
... homogeneous catalysts (acid-base or redox reaction mechanisms). Examples could include some proteolytic enzymes with specific activities, e.g. trypsin. A reversible reaction can take place in either direction. A dynamic equilibrium is characterised by the following: • it must occur in a closed syste ...
... homogeneous catalysts (acid-base or redox reaction mechanisms). Examples could include some proteolytic enzymes with specific activities, e.g. trypsin. A reversible reaction can take place in either direction. A dynamic equilibrium is characterised by the following: • it must occur in a closed syste ...
Chapter 10
... These molar ratios are used to 'convert' between any two compounds, whether they are reactants or products. This allows us to calculate moles of reactants needed, or products produced. ...
... These molar ratios are used to 'convert' between any two compounds, whether they are reactants or products. This allows us to calculate moles of reactants needed, or products produced. ...
Chapter 14 – Chemical Reactions
... Products – the substances _____________ as a _____________ of a chemical _____________ Coefficient – a _____________ placed in _____________ of a chemical _____________ or _____________ All chemical equations must be balanced. Steps to Balancing Chemical Equations: 1. Count the atoms of each element ...
... Products – the substances _____________ as a _____________ of a chemical _____________ Coefficient – a _____________ placed in _____________ of a chemical _____________ or _____________ All chemical equations must be balanced. Steps to Balancing Chemical Equations: 1. Count the atoms of each element ...
2011 Chem Facts Key
... 33. Ionic bonds form when one atom transfers an electron to another atom when forming a bond with it. Which substance exhibits ionic bonding rather than covalent bonding? CO2 , N2O4, SiO2 , CaBr2 , C6H12O6 34. Lewis Dot Diagrams may be used to represent the formation of polyatomic ions or covalent m ...
... 33. Ionic bonds form when one atom transfers an electron to another atom when forming a bond with it. Which substance exhibits ionic bonding rather than covalent bonding? CO2 , N2O4, SiO2 , CaBr2 , C6H12O6 34. Lewis Dot Diagrams may be used to represent the formation of polyatomic ions or covalent m ...
2014 Academic Challenge Sectional Chemistry Exam Solution Set 1
... B. Only the second molecule is polar. In the third and fourth structures, the square planar shape causes any bond dipoles to cancel out. ...
... B. Only the second molecule is polar. In the third and fourth structures, the square planar shape causes any bond dipoles to cancel out. ...
Chemistry 1 Revision: Metals and their uses
... Complete the following using the periodic table to help: H2O: ........... atoms of h.......................... .......... atoms of o....................... ...
... Complete the following using the periodic table to help: H2O: ........... atoms of h.......................... .......... atoms of o....................... ...
Balanced Chemical Equation
... 2. By inspection, find an element or polyatomic group that does not have equal amounts on both sides. 3. Add coefficients to make the number of atoms or groups equal on both sides of equation. ...
... 2. By inspection, find an element or polyatomic group that does not have equal amounts on both sides. 3. Add coefficients to make the number of atoms or groups equal on both sides of equation. ...
C1 Revision Fundamental ideas adapted CS
... Complete the following using the periodic table to help: H2O: ........... atoms of h.......................... .......... atoms of o....................... ...
... Complete the following using the periodic table to help: H2O: ........... atoms of h.......................... .......... atoms of o....................... ...
Final Review
... 4. What is the relationship between atmospheric pressure and the boiling point of a liquid? 5. Water has a high heat of fusion (6.009 KJ/mol) and a high heat of vaporization (40.79 KJ/mol). Explain what this means in terms of attraction between particles. 6. Using the values given in #5, calculate t ...
... 4. What is the relationship between atmospheric pressure and the boiling point of a liquid? 5. Water has a high heat of fusion (6.009 KJ/mol) and a high heat of vaporization (40.79 KJ/mol). Explain what this means in terms of attraction between particles. 6. Using the values given in #5, calculate t ...
Balancing ANY chemical Equation
... 2- Write the correct formula for the substance indicated 3- Replace each word “and”, “combine” or “plus” with the symbol “+” 4- Replace each phrase indicating change (make, produces, yield, etc.) with and arrow pointing toward the right. 5- Balance each equation ...
... 2- Write the correct formula for the substance indicated 3- Replace each word “and”, “combine” or “plus” with the symbol “+” 4- Replace each phrase indicating change (make, produces, yield, etc.) with and arrow pointing toward the right. 5- Balance each equation ...
The Egyptian American International School
... 2. Probability maps indicate the likelihood of finding the electron at a given point in space. 3. The size of an atom can be described by a surface that contains 90% of the total electron probability. 11.4 Electron Configurations and Atomic Properties Atomic energy levels are broken down into prin ...
... 2. Probability maps indicate the likelihood of finding the electron at a given point in space. 3. The size of an atom can be described by a surface that contains 90% of the total electron probability. 11.4 Electron Configurations and Atomic Properties Atomic energy levels are broken down into prin ...
Chemistry 30 Notes - Heat of Formation February 2nd
... Chemistry 30 will require you to remember this basic chemistry skill! Step 2: Determine kJ for 0.390 mol We know from the question that 297 kJ of energy is released for 1 mole of SO2 — the definition of heat of formation. Determine how much energy will be released for 0.390 mol of SO2: kJ released = ...
... Chemistry 30 will require you to remember this basic chemistry skill! Step 2: Determine kJ for 0.390 mol We know from the question that 297 kJ of energy is released for 1 mole of SO2 — the definition of heat of formation. Determine how much energy will be released for 0.390 mol of SO2: kJ released = ...
Lesson 1 - Working With Chemicals
... NH4+, which acts as a metal in compounds. - The name of the cation (metal) is followed by the name of the anion (non-metal – negatively ...
... NH4+, which acts as a metal in compounds. - The name of the cation (metal) is followed by the name of the anion (non-metal – negatively ...
Ionic bonding - Nidderdale High School
... other because there are no covalent bonds between the layers and so graphite is soft and ...
... other because there are no covalent bonds between the layers and so graphite is soft and ...
Resource for Final Exam Prep
... AgNO3(aq) + Cl–(aq) AgCl(aq) + NO3–(aq) What mass of chloride ion is present in a 100.0 g sample of aqueous solution if 40.8 mL of 0.100 M AgNO3 is required to react with all the chloride ion in the sample? 1) 4.08 10–3 g 2) 0.144 g ...
... AgNO3(aq) + Cl–(aq) AgCl(aq) + NO3–(aq) What mass of chloride ion is present in a 100.0 g sample of aqueous solution if 40.8 mL of 0.100 M AgNO3 is required to react with all the chloride ion in the sample? 1) 4.08 10–3 g 2) 0.144 g ...
The Chemical Earth
... Alter the coefficients to balance the number of each type of atom on both sides of the equation ...
... Alter the coefficients to balance the number of each type of atom on both sides of the equation ...
Chemical Equations
... Reaction Types: Synthesis or Composition • Synthesis are, at this introductory level, almost always the reverse of a decomposition reaction. That means that two pieces join together to produce one, a more complex compounds. These pieces can be elements or simpler compounds. • A + B ---> AB Reaction ...
... Reaction Types: Synthesis or Composition • Synthesis are, at this introductory level, almost always the reverse of a decomposition reaction. That means that two pieces join together to produce one, a more complex compounds. These pieces can be elements or simpler compounds. • A + B ---> AB Reaction ...
Chemistry Review
... BALANCING EQUATIONS: 4 steps: 1. Start with a word equation 2. Convert to a formula equation (don’t forget the diatomic molecules!) 3. Balance with coefficients: balance each atom one at a time balance polyatomic ions on each side of the equation as one unit balance H and O last (they often appear i ...
... BALANCING EQUATIONS: 4 steps: 1. Start with a word equation 2. Convert to a formula equation (don’t forget the diatomic molecules!) 3. Balance with coefficients: balance each atom one at a time balance polyatomic ions on each side of the equation as one unit balance H and O last (they often appear i ...
Redox
![](https://commons.wikimedia.org/wiki/Special:FilePath/NaF.gif?width=300)
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.