Document
... 1. Explain what is wrong with the statement “My friend burned a piece of paper (a hydrocarbon) that had the final exam on it and it disappeared”. (Be sure to use a chemical equation, identify reactants and product(s) and include energy). ANSWER: The paper (CxHy) was burned with oxygen and the atoms ...
... 1. Explain what is wrong with the statement “My friend burned a piece of paper (a hydrocarbon) that had the final exam on it and it disappeared”. (Be sure to use a chemical equation, identify reactants and product(s) and include energy). ANSWER: The paper (CxHy) was burned with oxygen and the atoms ...
atoms
... (a) Lithium nitrate Lithium (group 1A) forms only the Li+ ion and does not need a Roman numeral. (b) Potassium hydrogen sulfate (potassium bisulfate) Potassium (group 1A) forms only the K+ ion. (c) Copper(II) carbonate The carbonate ion has a 2 charge, so copper must be +2. A Roman numeral is neede ...
... (a) Lithium nitrate Lithium (group 1A) forms only the Li+ ion and does not need a Roman numeral. (b) Potassium hydrogen sulfate (potassium bisulfate) Potassium (group 1A) forms only the K+ ion. (c) Copper(II) carbonate The carbonate ion has a 2 charge, so copper must be +2. A Roman numeral is neede ...
1001_3rd Exam_1001214
... B) 34.5 kJ C) 40.4 kJ D) 68.9 kJ E) 185 kJ Answer: A 30) Why is the electron affinity so positive for the group 12 elements? A) The groups 12 elements are diatomic elements. B) The added electron would have to go into a new shell. C) The added electron would have to be added into the half-filled p s ...
... B) 34.5 kJ C) 40.4 kJ D) 68.9 kJ E) 185 kJ Answer: A 30) Why is the electron affinity so positive for the group 12 elements? A) The groups 12 elements are diatomic elements. B) The added electron would have to go into a new shell. C) The added electron would have to be added into the half-filled p s ...
Flexbook - What is Matter?
... substances present, each with the same properties that it had before it was mixed. When substances do not mix thoroughly and evenly (like sand and gravel), the mixture is said to be heterogeneous. A heterogeneous mixture consists of visibly different substances. Another example of a mixture is salt ...
... substances present, each with the same properties that it had before it was mixed. When substances do not mix thoroughly and evenly (like sand and gravel), the mixture is said to be heterogeneous. A heterogeneous mixture consists of visibly different substances. Another example of a mixture is salt ...
Identify the following properties as either - Teach-n-Learn-Chem
... 1. Explain what is wrong with the statement “My friend burned a piece of paper (a hydrocarbon) that had the final exam on it and it disappeared”. (Be sure to use a chemical equation, identify reactants and product(s) and include energy). ANSWER: The paper (CxHy) was burned with oxygen and the atoms ...
... 1. Explain what is wrong with the statement “My friend burned a piece of paper (a hydrocarbon) that had the final exam on it and it disappeared”. (Be sure to use a chemical equation, identify reactants and product(s) and include energy). ANSWER: The paper (CxHy) was burned with oxygen and the atoms ...
C:\usb key\sch3u\unit 1\chapter 2 test answers.wpd
... In a co-ordinate bond, both electrons come from the same atom. 2) Draw a Lewis diagram for the molecule HO. Label one of each of the following types of electrons: lone pair, bonded pair, and unpaired (3 points). ...
... In a co-ordinate bond, both electrons come from the same atom. 2) Draw a Lewis diagram for the molecule HO. Label one of each of the following types of electrons: lone pair, bonded pair, and unpaired (3 points). ...
Pre-AP Chemistry - Simple Rules for Electron Exchange Simple
... cases, we must do some electron bookkeeping. Oxidation numbers are the basis for electron bookkeeping. Tracking how they change as each chemical species goes from reactants to products helps us keep track of which species loses and which species gains electrons. You will note that oxidation numbers ...
... cases, we must do some electron bookkeeping. Oxidation numbers are the basis for electron bookkeeping. Tracking how they change as each chemical species goes from reactants to products helps us keep track of which species loses and which species gains electrons. You will note that oxidation numbers ...
Atom The smallest part of an element that can exist on its own
... Dibasic acid One which has 2 replaceable H atoms per molecule Isotopes Atoms having the same atomic number but different mass numbers - As the number of protons increases, the number of neutrons increases relatively faster, so small atoms have proton and neutron numbers which are comparable whereas ...
... Dibasic acid One which has 2 replaceable H atoms per molecule Isotopes Atoms having the same atomic number but different mass numbers - As the number of protons increases, the number of neutrons increases relatively faster, so small atoms have proton and neutron numbers which are comparable whereas ...
Worksheet 8 Notes - Department of Chemistry | Oregon State
... What is a Lewis base? What is a Lewis acid? Let me start by stating that we are familiar with many bases and acids. Those we know to be bases are Lewis bases and those we know to be acids are Lewis acids. Our previous ideas of bases and acids came from Arrhenius, Bronsted, and Lowry. These ideas inv ...
... What is a Lewis base? What is a Lewis acid? Let me start by stating that we are familiar with many bases and acids. Those we know to be bases are Lewis bases and those we know to be acids are Lewis acids. Our previous ideas of bases and acids came from Arrhenius, Bronsted, and Lowry. These ideas inv ...
Study Guide for Final #1
... 1.) Know who the important contributors were who helped to derive the different models of the atom. Know what their contributions were. 2.) Be able to describe Dalton’s atomic theory. 3.) Know where the three different subatomic particles are located, their charges, and their relative sizes. 4.) Kno ...
... 1.) Know who the important contributors were who helped to derive the different models of the atom. Know what their contributions were. 2.) Be able to describe Dalton’s atomic theory. 3.) Know where the three different subatomic particles are located, their charges, and their relative sizes. 4.) Kno ...
I. scientific notation. – a shorthand that scientists use when dealing
... Atomic weight – the relative masses of atoms of different elements that are proportional to the actual masses of atoms. amu – units of atomic weight. (atomic mass unit) 1 amu – 1/12 the mass of carbon-12. H 1 amu Mg 24.3 amu ...
... Atomic weight – the relative masses of atoms of different elements that are proportional to the actual masses of atoms. amu – units of atomic weight. (atomic mass unit) 1 amu – 1/12 the mass of carbon-12. H 1 amu Mg 24.3 amu ...
Term 1 and 2 Powerpoints
... something that expands outside of our classroom. Thinking about the candle burning sent me into deep contemplation. And then, out of complete randomness, I started thinking about our environment and the things that we burn which pollute it. I then thought of where all the statistics we hear about co ...
... something that expands outside of our classroom. Thinking about the candle burning sent me into deep contemplation. And then, out of complete randomness, I started thinking about our environment and the things that we burn which pollute it. I then thought of where all the statistics we hear about co ...
Balancing Chemical Equations – A Primer
... Sodium (Na) is found in Column #1. Na is element #11. This tells you that Na has 11+ protons and 11electrons with an overall charge of zero. In this column, elements have one electron in their valence shell. Na wants to get rid of that one electron. If it does, Na has 11+ charges and 10- charges for ...
... Sodium (Na) is found in Column #1. Na is element #11. This tells you that Na has 11+ protons and 11electrons with an overall charge of zero. In this column, elements have one electron in their valence shell. Na wants to get rid of that one electron. If it does, Na has 11+ charges and 10- charges for ...
CH2 Student Revision Guides pdf
... When hydrogen is covalently bonded to a very electronegative atom such as fluorine, nitrogen, oxygen, the covalent bond is very polar and the bonding pair of electrons drawn closely to the electronegative atom leaving an almost bare proton as the + end of the bond. This is attracted to any negative ...
... When hydrogen is covalently bonded to a very electronegative atom such as fluorine, nitrogen, oxygen, the covalent bond is very polar and the bonding pair of electrons drawn closely to the electronegative atom leaving an almost bare proton as the + end of the bond. This is attracted to any negative ...
CHAPTER 8 PERIODIC RELATIONSHIPS AMONG THE ELEMENTS
... right. A larger effective nuclear charge means a more tightly held outer electron, and hence a higher first ionization energy. Thus, in the third period, sodium has the lowest and neon has the highest first ionization energy. ...
... right. A larger effective nuclear charge means a more tightly held outer electron, and hence a higher first ionization energy. Thus, in the third period, sodium has the lowest and neon has the highest first ionization energy. ...
Instructor`s Guide - Ventura Educational Systems
... More often than not, atoms bond with other atoms to form molecules and compounds. Covalent Molecules, like water (H2O) and ethanol (CH3CH2OH), form when valence electron from one atom are shared with valence electrons from a second atom to form a Covalent Bond. Forming covalent bonds lowers the pote ...
... More often than not, atoms bond with other atoms to form molecules and compounds. Covalent Molecules, like water (H2O) and ethanol (CH3CH2OH), form when valence electron from one atom are shared with valence electrons from a second atom to form a Covalent Bond. Forming covalent bonds lowers the pote ...
CHAPTER 2: ATOMS, MOLECULES AND IONS ULES AND IONS
... 1. From left to right (row of periodic table) the atomic number (Number of protons) increases. 2. From top to bottom (vertical column of periodic table), the elements have similar chemical properties. ...
... 1. From left to right (row of periodic table) the atomic number (Number of protons) increases. 2. From top to bottom (vertical column of periodic table), the elements have similar chemical properties. ...
CHAPTER TEN MOLECULAR GEOMETRY MOLECULAR
... VALENCE BOND THEORY Hybridization – mixing of two or more atomic orbitals to form a new set of hybrid orbitals. 1. Mix at least 2 nonequivalent atomic orbitals (e.g. s and p). Hybrid orbitals have very different shape from original atomic orbitals. 2. Number of hybrid orbitals is equal to number of ...
... VALENCE BOND THEORY Hybridization – mixing of two or more atomic orbitals to form a new set of hybrid orbitals. 1. Mix at least 2 nonequivalent atomic orbitals (e.g. s and p). Hybrid orbitals have very different shape from original atomic orbitals. 2. Number of hybrid orbitals is equal to number of ...
Subject Area Assessment Guides
... A few other groups are given family names. These include the alkali metals (Group 1), such as sodium and potassium, which are soft and white and extremely reactive chemically. Alkaline earth metals (Group 2), such as magnesium and calcium, are found in the second column of the periodic table. The tr ...
... A few other groups are given family names. These include the alkali metals (Group 1), such as sodium and potassium, which are soft and white and extremely reactive chemically. Alkaline earth metals (Group 2), such as magnesium and calcium, are found in the second column of the periodic table. The tr ...
inorganic chemistry
... the fact that the atoms of these elements have only one electron less than the stable noble gas (ns2np6) configurations. Therefore, may have maximum tendency to accept an additional electron. (ii) In general, electron affinity decreases from top to bottom in a group. This is due to the fact that the ...
... the fact that the atoms of these elements have only one electron less than the stable noble gas (ns2np6) configurations. Therefore, may have maximum tendency to accept an additional electron. (ii) In general, electron affinity decreases from top to bottom in a group. This is due to the fact that the ...
Regents Chemistry Topic Review Packet
... You need to know how to do the calculation of “weighted atomic mass” given isotope masses and percent abundances. 14. When an atom gains an electron, it becomes a negative ion and its radius increases. 15. When an atom loses an electron, it becomes a positive ion and its radius decreases. 16. Elec ...
... You need to know how to do the calculation of “weighted atomic mass” given isotope masses and percent abundances. 14. When an atom gains an electron, it becomes a negative ion and its radius increases. 15. When an atom loses an electron, it becomes a positive ion and its radius decreases. 16. Elec ...
Regents Chemistry Topic Review Packet
... You need to know how to do the calculation of “weighted atomic mass” given isotope masses and percent abundances. 14. When an atom gains an electron, it becomes a negative ion and its radius increases. 15. When an atom loses an electron, it becomes a positive ion and its radius decreases. 16. Elec ...
... You need to know how to do the calculation of “weighted atomic mass” given isotope masses and percent abundances. 14. When an atom gains an electron, it becomes a negative ion and its radius increases. 15. When an atom loses an electron, it becomes a positive ion and its radius decreases. 16. Elec ...
Glossary: Chemical bonds
... A chemical change is a dissociation, recombination, or rearrangement of atoms. compound Compare with element and mixture. A compound is a material formed from elements chemically combined in definite proportions by mass. For example, water is formed from chemically bound hydrogen and oxygen. Any pur ...
... A chemical change is a dissociation, recombination, or rearrangement of atoms. compound Compare with element and mixture. A compound is a material formed from elements chemically combined in definite proportions by mass. For example, water is formed from chemically bound hydrogen and oxygen. Any pur ...
Electronegativity
Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself. An atom's electronegativity is affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus. The higher the associated electronegativity number, the more an element or compound attracts electrons towards it. The term ""electronegativity"" was introduced by Jöns Jacob Berzelius in 1811,though the concept was known even before that and was studied by many chemists including Avogadro.In spite of its long history, an accurate scale of electronegativity had to wait till 1932, when Linus Pauling proposed an electronegativity scale, which depends on bond energies, as a development of valence bond theory. It has been shown to correlate with a number of other chemical properties. Electronegativity cannot be directly measured and must be calculated from other atomic or molecular properties. Several methods of calculation have been proposed, and although there may be small differences in the numerical values of the electronegativity, all methods show the same periodic trends between elements. The most commonly used method of calculation is that originally proposed by Linus Pauling. This gives a dimensionless quantity, commonly referred to as the Pauling scale, on a relative scale running from around 0.7 to 3.98 (hydrogen = 2.20). When other methods of calculation are used, it is conventional (although not obligatory) to quote the results on a scale that covers the same range of numerical values: this is known as an electronegativity in Pauling units. As it is usually calculated, electronegativity is not a property of an atom alone, but rather a property of an atom in a molecule. Properties of a free atom include ionization energy and electron affinity. It is to be expected that the electronegativity of an element will vary with its chemical environment, but it is usually considered to be a transferable property, that is to say that similar values will be valid in a variety of situations.On the most basic level, electronegativity is determined by factors like the nuclear charge (the more protons an atom has, the more ""pull"" it will have on electrons) and the number/location of other electrons present in the atomic shells (the more electrons an atom has, the farther from the nucleus the valence electrons will be, and as a result the less positive charge they will experience—both because of their increased distance from the nucleus, and because the other electrons in the lower energy core orbitals will act to shield the valence electrons from the positively charged nucleus).The opposite of electronegativity is electropositivity: a measure of an element's ability to donate electrons.Caesium is the least electronegative element in the periodic table (=0.79), while fluorine is most electronegative (=3.98). (Francium and caesium were originally assigned both assigned 0.7; caesium's value was later refined to 0.79, but no experimental data allows a similar refinement for francium. However, francium's ionization energy is known to be slightly higher than caesium's, in accordance with the relativistic stabilization of the 7s orbital, and this in turn implies that caesium is in fact more electronegative than francium.)