Chapter 2
... (1+ ions only). Neon consists of three isotopes, of which neon-20 is by far the most abundant (90.48%). The mass of that isotope, to five decimal places, is 19.99244 amu on the carbon-12 scale. The number by each peak corresponds to the fraction of all Ne+ ions represented by the isotope with that m ...
... (1+ ions only). Neon consists of three isotopes, of which neon-20 is by far the most abundant (90.48%). The mass of that isotope, to five decimal places, is 19.99244 amu on the carbon-12 scale. The number by each peak corresponds to the fraction of all Ne+ ions represented by the isotope with that m ...
6CH02 - MPPE
... Answer ALL the questions. Write your answers in the spaces provided. 17 This question is about the element chlorine and its compounds. (a) When chlorine is bubbled through water, a solution of chlorine water forms. What is the colour of chlorine water? ...
... Answer ALL the questions. Write your answers in the spaces provided. 17 This question is about the element chlorine and its compounds. (a) When chlorine is bubbled through water, a solution of chlorine water forms. What is the colour of chlorine water? ...
Writing Chemical Formulas
... Since electrons have a negative charge, and atom with a negative oxidation number will gain electrons. That means an atom with a positive oxidation number will lose electrons. Nonmetals and polyatomic ions almost always gain electrons - have negative oxidation numbers. Metals almost always lose elec ...
... Since electrons have a negative charge, and atom with a negative oxidation number will gain electrons. That means an atom with a positive oxidation number will lose electrons. Nonmetals and polyatomic ions almost always gain electrons - have negative oxidation numbers. Metals almost always lose elec ...
Unit 1: Basic Chemistry for Biology QUIZ STUDY GUIDE Things to
... -Know the difference between a covalent bond and an ionic bond. -Be able to answer questions about a bond similar to the ones on ...
... -Know the difference between a covalent bond and an ionic bond. -Be able to answer questions about a bond similar to the ones on ...
A-level Chemistry Modified question paper Unit 01
... phosphoric acid in this solution. [5 marks] Give your answer to 3 significant figures. ...
... phosphoric acid in this solution. [5 marks] Give your answer to 3 significant figures. ...
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 ...
9.1 Electron Transfer Reactions
... certain rules • An atom’s oxidation number is the positive or negative charge on the atom if the electron pairs in a covalent bond belong only to the more electronegative atom ...
... certain rules • An atom’s oxidation number is the positive or negative charge on the atom if the electron pairs in a covalent bond belong only to the more electronegative atom ...
Stoichiometry - hrsbstaff.ednet.ns.ca
... illustrate and explain the formation of ionic, covalent, and metallic bonds determine the distribution of electrons in the major energy levels for the first thirtyeighth elements and for ions in groups 1, 2, 3, 15, 16, and 17 state the octet rule predict the ionic charge for ions in the main ...
... illustrate and explain the formation of ionic, covalent, and metallic bonds determine the distribution of electrons in the major energy levels for the first thirtyeighth elements and for ions in groups 1, 2, 3, 15, 16, and 17 state the octet rule predict the ionic charge for ions in the main ...
AP Chemistry Second Semester Notes
... 2. form molecules in addition to ionic compounds a. E to remove electron from a gaseous atom 3. large positive ionization energy 1. X(g) X+(g) + 1e4. large negative electron affinity except 2. all +E (greater value = harder to ionize) columns 15 and 18 b. inversely proportional to atomic radius ...
... 2. form molecules in addition to ionic compounds a. E to remove electron from a gaseous atom 3. large positive ionization energy 1. X(g) X+(g) + 1e4. large negative electron affinity except 2. all +E (greater value = harder to ionize) columns 15 and 18 b. inversely proportional to atomic radius ...
effective nuclear charge
... Trends in Ionic Radius Ions in same group have same charge Ion size increases down the group higher valence shell, larger ...
... Trends in Ionic Radius Ions in same group have same charge Ion size increases down the group higher valence shell, larger ...
chemistry in the 8th grade
... space. Scientists use a system to classify matter based on its composition and purity. Matter in its purest form comes in two types – elements and compounds. The simplest form of matter is an element. An element is composed of a single kind of atom. Gold would be an example of an element, as it is c ...
... space. Scientists use a system to classify matter based on its composition and purity. Matter in its purest form comes in two types – elements and compounds. The simplest form of matter is an element. An element is composed of a single kind of atom. Gold would be an example of an element, as it is c ...
Original
... The energy of ionic bonds can be calculated using Coulomb’s Law, where Q = the charge of each ion, and r = distance between ions (nm): (Negative answer = attraction, positive answer = repulsion) E = 2.31x10-19 J nm (Q1Q2/r) For example, the energy of a NaCl bond, given r = 0.276nm, would be: 2.31x10 ...
... The energy of ionic bonds can be calculated using Coulomb’s Law, where Q = the charge of each ion, and r = distance between ions (nm): (Negative answer = attraction, positive answer = repulsion) E = 2.31x10-19 J nm (Q1Q2/r) For example, the energy of a NaCl bond, given r = 0.276nm, would be: 2.31x10 ...
Chapter 10 Molecular Geometry and Chemical Bonding Theory
... Lewis theory (Ch. 9): covalent bond forms when an electron pair is shared between 2 atoms. Valence Bond Theory: concentration of electron density between atoms occurs when a valence atomic orbital on one atom overlaps with the valence atomic orbital on the other atom. ...
... Lewis theory (Ch. 9): covalent bond forms when an electron pair is shared between 2 atoms. Valence Bond Theory: concentration of electron density between atoms occurs when a valence atomic orbital on one atom overlaps with the valence atomic orbital on the other atom. ...
Chapter 07 and 08 Chemical Bonding and Molecular
... • Made of 2 or more elements in a definite proportion by mass • Physically and chemically different from the elements that make up the compound • All elements (except Noble gases) react to gain a stable octet. (duet-for H through B) • Compounds form to gain a stable valence shell which is LOWER IN E ...
... • Made of 2 or more elements in a definite proportion by mass • Physically and chemically different from the elements that make up the compound • All elements (except Noble gases) react to gain a stable octet. (duet-for H through B) • Compounds form to gain a stable valence shell which is LOWER IN E ...
Syracuse University
... courses intended for students with an interest or background in science. No prior chemistry instruction is required or assumed. A general, basic understanding of math and algebra, including an understanding of decimals, exponents, logarithms, quadratics, and algebraic equations, is essential to succ ...
... courses intended for students with an interest or background in science. No prior chemistry instruction is required or assumed. A general, basic understanding of math and algebra, including an understanding of decimals, exponents, logarithms, quadratics, and algebraic equations, is essential to succ ...
Chapter 7-8-9
... Which of the following pairs of elements is most likely to form a covalent compound? a. magnesium and c. oxygen and chlorine fluorine d. sodium and b. lithium and bromine aluminuim Which is a physical property of ionic compounds in their solid state? a. good conductor of electricity b. weak attracti ...
... Which of the following pairs of elements is most likely to form a covalent compound? a. magnesium and c. oxygen and chlorine fluorine d. sodium and b. lithium and bromine aluminuim Which is a physical property of ionic compounds in their solid state? a. good conductor of electricity b. weak attracti ...
Which notation represents an atom of sodium
... A hydrate is a compound that has water molecules within its crystal structure. The formula for the hydrate CuSO4•5H2O(s) shows that there are five moles of water for every one mole of CuSO4(s). When CuSO4•5H2O(s) is heated, the water within the crystals is released, as represented by the balanced eq ...
... A hydrate is a compound that has water molecules within its crystal structure. The formula for the hydrate CuSO4•5H2O(s) shows that there are five moles of water for every one mole of CuSO4(s). When CuSO4•5H2O(s) is heated, the water within the crystals is released, as represented by the balanced eq ...
PART 2 – CHEMISTRY
... If the outer energy level or shell is incomplete, having less than the numbers stated above, the atom is said to be chemically unstable. These atoms tend to react with other atoms until they reach an external energy level of 2 or 8 electrons, thus becoming a stable compound. Chemical Bonds. The forc ...
... If the outer energy level or shell is incomplete, having less than the numbers stated above, the atom is said to be chemically unstable. These atoms tend to react with other atoms until they reach an external energy level of 2 or 8 electrons, thus becoming a stable compound. Chemical Bonds. The forc ...
Chem. 121, Sec 11 Name: Student I.D. Please Show Your Work
... D) I, II, and III E) I, II, III, and IV 12. Calculate the energy required to promote an electron in a hydrogen atom from a 4f to a 5s orbital. (4 marks) ...
... D) I, II, and III E) I, II, III, and IV 12. Calculate the energy required to promote an electron in a hydrogen atom from a 4f to a 5s orbital. (4 marks) ...
Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures
... Unit 2: Atoms, experiments, p+, n0, e-, ions, isotopes, nuclear equations 1. What is the name of Dalton’s model of the atom? a. Plum pudding model b. Quantum mechanical model c. Nuclear model d. Solid sphere model 2. What is the name of J.J. Thompson’s model of the atom? a. Plum pudding model b. Qu ...
... Unit 2: Atoms, experiments, p+, n0, e-, ions, isotopes, nuclear equations 1. What is the name of Dalton’s model of the atom? a. Plum pudding model b. Quantum mechanical model c. Nuclear model d. Solid sphere model 2. What is the name of J.J. Thompson’s model of the atom? a. Plum pudding model b. Qu ...
Chemistry SOL Review
... • To determine whether a bond is polar, nonpolar, or ionic, you must use a table of electronegativities. (This will be given to you on the SOL if you are supposed to use it.) When you subtract the two values, if the difference is… – …between 0 and 0.4, the bond is nonpolar, meaning the electrons are ...
... • To determine whether a bond is polar, nonpolar, or ionic, you must use a table of electronegativities. (This will be given to you on the SOL if you are supposed to use it.) When you subtract the two values, if the difference is… – …between 0 and 0.4, the bond is nonpolar, meaning the electrons are ...
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.)