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4.1 PPT- Atomic Theory and Bonding
... Atoms gain and lose electrons in an attempt to be STABLE. The noble gases are stable because they have FULL outer shells of electrons. They don’t need to lose or gain any e-s. Atoms in each period want to have the same number of electrons in their outer shell (VALENCE ELECTRONS) as the noble gases ...
... Atoms gain and lose electrons in an attempt to be STABLE. The noble gases are stable because they have FULL outer shells of electrons. They don’t need to lose or gain any e-s. Atoms in each period want to have the same number of electrons in their outer shell (VALENCE ELECTRONS) as the noble gases ...
Homework Exercises
... What is meant by an excess of one chemical in a chemical reaction? When the reaction is finished, unreacted copper(II) carbonate would be left in the beaker. What else would be observed indicating that the reaction is over? (e) Draw a labelled diagram of the apparatus you would use to remove the unr ...
... What is meant by an excess of one chemical in a chemical reaction? When the reaction is finished, unreacted copper(II) carbonate would be left in the beaker. What else would be observed indicating that the reaction is over? (e) Draw a labelled diagram of the apparatus you would use to remove the unr ...
Unit 6 Worksheet Package
... the sharing or transfer of ____________ between pairs of atoms. Bonded atoms attain the stable electron configuration of a __________ ______. The transfer of valence electrons produces positively charged ions, or _____________, and negatively charged ions called _____________. The attraction between ...
... the sharing or transfer of ____________ between pairs of atoms. Bonded atoms attain the stable electron configuration of a __________ ______. The transfer of valence electrons produces positively charged ions, or _____________, and negatively charged ions called _____________. The attraction between ...
MT 3 Practice
... No precipitate formed. Ammonium carbonate was added and a precipitate formed. The precipitate was then dissolved by the addition of HCl. Sodium sulfate was then added and a precipitate formed. What is the identity of the cation. [A] Co2+ [B] Ca2+ [C] Ba2+ [D] Ni2+ 2. 1M NH3 was added to to a solutio ...
... No precipitate formed. Ammonium carbonate was added and a precipitate formed. The precipitate was then dissolved by the addition of HCl. Sodium sulfate was then added and a precipitate formed. What is the identity of the cation. [A] Co2+ [B] Ca2+ [C] Ba2+ [D] Ni2+ 2. 1M NH3 was added to to a solutio ...
Question 2
... 1. Small quantities of hydrogen gas can be prepared in the laboratory by the following reaction: Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) Assume you carried out this experiment and collected 653 mL of hydrogen gas over water. The gas mixture collected includes hydrogen and water vapor. The temperature ...
... 1. Small quantities of hydrogen gas can be prepared in the laboratory by the following reaction: Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) Assume you carried out this experiment and collected 653 mL of hydrogen gas over water. The gas mixture collected includes hydrogen and water vapor. The temperature ...
Reactions I Can..
... the relative mass composition of the constituent elements. 10. Calculate the molecular formula of a compound given the empirical formula and the molecular mass. 11. Summarize how the gas variables of P, V, n, And T relate to each other in common situations such as the air in a car tire or the air in ...
... the relative mass composition of the constituent elements. 10. Calculate the molecular formula of a compound given the empirical formula and the molecular mass. 11. Summarize how the gas variables of P, V, n, And T relate to each other in common situations such as the air in a car tire or the air in ...
Atoms
... metals, alkaline earth metals, halogens, noble gases, lanthanide series, actinide series, transition elements, inner-transition elements, and trans-uranic elements. 6. Identify the phase (solid, liquid, gas) of each element on the Periodic Table. 7. Explain the basic periodic trends of radius and io ...
... metals, alkaline earth metals, halogens, noble gases, lanthanide series, actinide series, transition elements, inner-transition elements, and trans-uranic elements. 6. Identify the phase (solid, liquid, gas) of each element on the Periodic Table. 7. Explain the basic periodic trends of radius and io ...
600 $600
... positively-charged particles A. Passed unchanged through gold foil. B. Changed directions as they passed through gold foil. C. Were stopped by gold foil. D. Bounced back after striking gold foil. ...
... positively-charged particles A. Passed unchanged through gold foil. B. Changed directions as they passed through gold foil. C. Were stopped by gold foil. D. Bounced back after striking gold foil. ...
Atoms and Molecules
... type of ions involved not how many of each ion cations: name the element; if more than one oxidation state is possible (d-block) follow with the charge in Roman numerals in parentheses anions: if monatomic then use the elemental name but with an –ide ending if polyatomic then use the memorized name ...
... type of ions involved not how many of each ion cations: name the element; if more than one oxidation state is possible (d-block) follow with the charge in Roman numerals in parentheses anions: if monatomic then use the elemental name but with an –ide ending if polyatomic then use the memorized name ...
Smith Reaction- HW PSI Chemistry
... C) The starting materials are named reactants. D) The bonds of the reactants are broken and new bonds of the products are formed. E) In a word equation representing a chemical reaction, the reactants are written on the left and the products on the right. 14) Chemical equations _____. A) describe che ...
... C) The starting materials are named reactants. D) The bonds of the reactants are broken and new bonds of the products are formed. E) In a word equation representing a chemical reaction, the reactants are written on the left and the products on the right. 14) Chemical equations _____. A) describe che ...
ch-4-earth-chemistry
... Example: A neutral sodium atom has a charge of zero (equal # of protons and neutrons) and only 1 valence electron. Once it loses that valence electron, it will have 8 valence electrons and be stable and most likely, not gain or lose anymore electrons. What would be the charge on a sodium atom that l ...
... Example: A neutral sodium atom has a charge of zero (equal # of protons and neutrons) and only 1 valence electron. Once it loses that valence electron, it will have 8 valence electrons and be stable and most likely, not gain or lose anymore electrons. What would be the charge on a sodium atom that l ...
form revision a
... Check your key area statements. If not green you need to do more work! Knowledge of the structure of the periodic table, groups and periods. All matter is made of atoms. When a substance contains only one kind of atom it is known as an element. Atoms contain protons, neutrons and electrons each with ...
... Check your key area statements. If not green you need to do more work! Knowledge of the structure of the periodic table, groups and periods. All matter is made of atoms. When a substance contains only one kind of atom it is known as an element. Atoms contain protons, neutrons and electrons each with ...
PPT - George Mason University
... electrons make it a good electrical conductor Although Aluminum is a metal, its halides exist in the gaseous state as covalent dimers - AL2Cl6 (contrast salts of group 1 & 2 metals) Aluminum Oxide, Al2O3, is amphoteric (can act as an acid or base) rather than basic like the Group 1A & 2A metals Alth ...
... electrons make it a good electrical conductor Although Aluminum is a metal, its halides exist in the gaseous state as covalent dimers - AL2Cl6 (contrast salts of group 1 & 2 metals) Aluminum Oxide, Al2O3, is amphoteric (can act as an acid or base) rather than basic like the Group 1A & 2A metals Alth ...
S294 Are you Ready for S294 e1i1 web029856
... The study of this module provides a solid foundation on which to build a life science specialism. S294 is a recommended stepping stone to the Level 3 Biology and Health Sciences modules, particularly S377 and SK320. If you are intending to study S294, you will want to make sure that you have the nec ...
... The study of this module provides a solid foundation on which to build a life science specialism. S294 is a recommended stepping stone to the Level 3 Biology and Health Sciences modules, particularly S377 and SK320. If you are intending to study S294, you will want to make sure that you have the nec ...
Name……………………………………............................. Index number
... Write your name, index number class and admission number in the spaces provided Sign and write the date of examination in the spaces provided. Answer all the questions in the spaces provided. Mathematical tables and silent electronic calculators may be used. All working must be clearly shown where n ...
... Write your name, index number class and admission number in the spaces provided Sign and write the date of examination in the spaces provided. Answer all the questions in the spaces provided. Mathematical tables and silent electronic calculators may be used. All working must be clearly shown where n ...
Chemical Equations
... Single replacement reactions are also called substitution reactions They have the form A + BX → B + AX, where A and B are elements and BX and AX are compounds ...
... Single replacement reactions are also called substitution reactions They have the form A + BX → B + AX, where A and B are elements and BX and AX are compounds ...
Language of chemistry
... H2O. That means there are 2 hydrogen atoms combining with 1 oxygen atom. Why is this? It is because oxygen has a valency of 2 while hydrogen has a valency of 1. How do we remember this? For now it will help to remember a few valencies. Monovalent Divalent Trivalent Tetra valent H - hydrogen Ca - cal ...
... H2O. That means there are 2 hydrogen atoms combining with 1 oxygen atom. Why is this? It is because oxygen has a valency of 2 while hydrogen has a valency of 1. How do we remember this? For now it will help to remember a few valencies. Monovalent Divalent Trivalent Tetra valent H - hydrogen Ca - cal ...
CHEM 481. Assignment 0. Review of General Chemistry. Answers
... 4. What is the difference between a group and a period in the periodic table? The groups are the vertical columns; the periods the horizontal rows. The groups collect elements that have similarities in chemical properties because the rows are repeating sequences of valence electron configurations - ...
... 4. What is the difference between a group and a period in the periodic table? The groups are the vertical columns; the periods the horizontal rows. The groups collect elements that have similarities in chemical properties because the rows are repeating sequences of valence electron configurations - ...
Chemistry I Exams and Answer Keys 2015 Season
... A pure metal is made up of atoms that are held together by all valence electrons that are not held exclusively by any particular atoms, but move freely around them. This statement is best described as A. a correct definition of a chemical term or expression, either in terms of experimental behavior ...
... A pure metal is made up of atoms that are held together by all valence electrons that are not held exclusively by any particular atoms, but move freely around them. This statement is best described as A. a correct definition of a chemical term or expression, either in terms of experimental behavior ...
Answers to Assignment #1
... 5. Name and give symbols for (a) three elements that are metals, (b) four elements that are nonmetals, (c) and two elements that are metalloids. In each case locate the element in the periodic table by giving the group and period in which the element is found. Metalloids are: B, Si, Ge, As, Sb, Te; ...
... 5. Name and give symbols for (a) three elements that are metals, (b) four elements that are nonmetals, (c) and two elements that are metalloids. In each case locate the element in the periodic table by giving the group and period in which the element is found. Metalloids are: B, Si, Ge, As, Sb, Te; ...
Aps midREVIEW
... 17. When the pressure exerted on a confined gas at constant temperature is doubled, the volume of the gas is A. halved B. doubled C. tripled D. quartered 18. Which is an example of a binary compound? A. acetic acid B. nitric acid C. potassium hydroxide D. potassium oxide 19. The volume ...
... 17. When the pressure exerted on a confined gas at constant temperature is doubled, the volume of the gas is A. halved B. doubled C. tripled D. quartered 18. Which is an example of a binary compound? A. acetic acid B. nitric acid C. potassium hydroxide D. potassium oxide 19. The volume ...
Chapter 4: Solution Chemistry: The Hydrosphere
... – One reactant Loses Electrons/is Oxidized (LEO) – Another reactant Gains Electrons/is Reduced (GER) An easy way to remember is “LEO the lion goes GER!” – The element or reactant that is oxidized is the reducing agent. – The element or reactant that is reduced is the oxidizing agent. CHEM 161: ...
... – One reactant Loses Electrons/is Oxidized (LEO) – Another reactant Gains Electrons/is Reduced (GER) An easy way to remember is “LEO the lion goes GER!” – The element or reactant that is oxidized is the reducing agent. – The element or reactant that is reduced is the oxidizing agent. CHEM 161: ...
Science24-UnitA-Section3.4
... you get a chemical equation. Chemical equations are used to represent all reactions. In mathematics you work with equations. What you do to one side of the equation must be done to the other side to keep the equation balanced. Similarly, in chemical equations you need have the same number of atoms o ...
... you get a chemical equation. Chemical equations are used to represent all reactions. In mathematics you work with equations. What you do to one side of the equation must be done to the other side to keep the equation balanced. Similarly, in chemical equations you need have the same number of atoms o ...
Synthesis of Alum Lab
... d) Alum forms from potassium ions, hydrated aluminum ions sulfate ions and water: K+(aq) + 6H2O(l) + 2SO42-(aq) + [Al(H2O)6]3+(aq) KAl(SO4)2.12H2O(s) ...
... d) Alum forms from potassium ions, hydrated aluminum ions sulfate ions and water: K+(aq) + 6H2O(l) + 2SO42-(aq) + [Al(H2O)6]3+(aq) KAl(SO4)2.12H2O(s) ...
Redox
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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.