Chapter 2 – Chemical Composition of the Body
... important because they alter the physical and chemical properties of many molecules (especially water).. ...
... important because they alter the physical and chemical properties of many molecules (especially water).. ...
CHM 2045C - State College of Florida
... This course meets Area V for the A.A./A.S. general education requirements. A rigorous study of chemistry principles for students who have already studied basic concepts of chemistry. This course is intended for science and science-related majors. ...
... This course meets Area V for the A.A./A.S. general education requirements. A rigorous study of chemistry principles for students who have already studied basic concepts of chemistry. This course is intended for science and science-related majors. ...
chemistry i
... decreases. The equation E = hν means that as frequency increases, energy increases. Using this information and the reference tables, which color of visible light has the least energy? A. Red b. Yellow c. Green d. Violet 38. If an electron drops from n=6 to n=2, what type of electromagnetic radiation ...
... decreases. The equation E = hν means that as frequency increases, energy increases. Using this information and the reference tables, which color of visible light has the least energy? A. Red b. Yellow c. Green d. Violet 38. If an electron drops from n=6 to n=2, what type of electromagnetic radiation ...
General Chemistry First Semester Review General
... - aqueous (aq) is written if a solution is used - pure liquids (not a mixture of something) use (l) - solid: This could refer to a multitude of different substances: metals, flakes, crystals, and precipitates; use (s) - gas: Use (g), these are usually diatomic molecules such as O2, H2, Cl2, etc. - r ...
... - aqueous (aq) is written if a solution is used - pure liquids (not a mixture of something) use (l) - solid: This could refer to a multitude of different substances: metals, flakes, crystals, and precipitates; use (s) - gas: Use (g), these are usually diatomic molecules such as O2, H2, Cl2, etc. - r ...
Name________________________ Midterm Review Date
... 56. A sample of a compound contains 65.4 grams of zinc, 12.0 grams of carbon, and 48.0 grams of oxygen. What is the mole ratio of zinc to carbon to oxygen in this compound? A) 1:4:6 C) 5:1:4 ...
... 56. A sample of a compound contains 65.4 grams of zinc, 12.0 grams of carbon, and 48.0 grams of oxygen. What is the mole ratio of zinc to carbon to oxygen in this compound? A) 1:4:6 C) 5:1:4 ...
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... A) Hydrogen provides a pair of electrons to be shared with nitrogen. B) Nitrogen provides a pair of electrons to be shared with hydrogen. C) Hydrogen transfers a pair of electrons to nitrogen. D) Nitrogen transfers a pair of electrons to hydrogen. 29. Which type of bond would be formed when a hydrog ...
... A) Hydrogen provides a pair of electrons to be shared with nitrogen. B) Nitrogen provides a pair of electrons to be shared with hydrogen. C) Hydrogen transfers a pair of electrons to nitrogen. D) Nitrogen transfers a pair of electrons to hydrogen. 29. Which type of bond would be formed when a hydrog ...
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... • Anion: an atom that carries a negative charge because it has more electrons than protons • Cation: an atom that carries a positive charge because it has more protons than electrons ...
... • Anion: an atom that carries a negative charge because it has more electrons than protons • Cation: an atom that carries a positive charge because it has more protons than electrons ...
Ionic and Covalent Bonding
... • the electrons in the highest occupied energy level of an element’s atom ...
... • the electrons in the highest occupied energy level of an element’s atom ...
Chapter 4: Introduction to Earth Chemistry Section 1 Notes
... Because isotopes of an element have different ____________, the periodic table uses an average atomic mass of each element. The average atomic mass is the ___________ average of the atomic masses of the naturally occurring isotopes of an element. Valence Electrons and Periodic Properties Based on si ...
... Because isotopes of an element have different ____________, the periodic table uses an average atomic mass of each element. The average atomic mass is the ___________ average of the atomic masses of the naturally occurring isotopes of an element. Valence Electrons and Periodic Properties Based on si ...
chemistry i - surrattchemistry
... 31. Which substance would have London dispersion forces as the main type of intermolecular forces of attraction? a. H2O b. F2 d. HCl d. NaCl 32. Diamond, graphite, and silicon dioxide all exhibit which type of intermolecular force? a. metallic b. network covalent c. ionic d. hydrogen e. dipole-dipol ...
... 31. Which substance would have London dispersion forces as the main type of intermolecular forces of attraction? a. H2O b. F2 d. HCl d. NaCl 32. Diamond, graphite, and silicon dioxide all exhibit which type of intermolecular force? a. metallic b. network covalent c. ionic d. hydrogen e. dipole-dipol ...
Name - Net Start Class
... C, B, A, D 6. Define viscosity and tell which of the following liquids would have the greatest viscosity. a. Definition - a property related to the resistance of a fluid to flow ...
... C, B, A, D 6. Define viscosity and tell which of the following liquids would have the greatest viscosity. a. Definition - a property related to the resistance of a fluid to flow ...
The Chemical Basis of Life
... – Different forms of an element with the same atomic number but with different mass numbers – The atoms of some isotopes are stable – Other isotopes are radioactive, having unstable atoms that spontaneously break apart (decay) to form other atoms – When radioactive atoms decay, energy is released ...
... – Different forms of an element with the same atomic number but with different mass numbers – The atoms of some isotopes are stable – Other isotopes are radioactive, having unstable atoms that spontaneously break apart (decay) to form other atoms – When radioactive atoms decay, energy is released ...
Chapter 9 - Fayetteville State University
... are the alkali metals (Li, Na, K, Rb, Cs), the halogens (F, Cl, Br, I). 8) Groups: A sequence of elements of increasing atomic number in the periodic table that share similar chemical properties (Example: group 1A Li, Na, K, Rb, Cs) 9) Metals: are characterized for having extra electrons outside the ...
... are the alkali metals (Li, Na, K, Rb, Cs), the halogens (F, Cl, Br, I). 8) Groups: A sequence of elements of increasing atomic number in the periodic table that share similar chemical properties (Example: group 1A Li, Na, K, Rb, Cs) 9) Metals: are characterized for having extra electrons outside the ...
What do we call a substance with more than one kind of atom
... 42. Within a period, the atomic radius __________ as the atomic number increases. 43. As a nonmetal becomes an ion, its radius _________ 44. The ______________ are the family that contain the most reactive metals. 45. Examine the following electron configuration for element X and use it to answer th ...
... 42. Within a period, the atomic radius __________ as the atomic number increases. 43. As a nonmetal becomes an ion, its radius _________ 44. The ______________ are the family that contain the most reactive metals. 45. Examine the following electron configuration for element X and use it to answer th ...
ViewpointAPBiology
... Two atoms can share more than one pair of electrons – double bonds (2 pairs of electrons) – triple bonds (3 pairs of electrons) ...
... Two atoms can share more than one pair of electrons – double bonds (2 pairs of electrons) – triple bonds (3 pairs of electrons) ...
Unit Description - Honors Chemistry
... orbital diagrams of the elements (5.3) Relate valence electrons to Lewis (electron dot) structures (5.3) Describe the ground-state arrangement of electrons in atoms of any element using orbital notation, electron configuration, and Lewis structures (5.3) Identify electron configuration that co ...
... orbital diagrams of the elements (5.3) Relate valence electrons to Lewis (electron dot) structures (5.3) Describe the ground-state arrangement of electrons in atoms of any element using orbital notation, electron configuration, and Lewis structures (5.3) Identify electron configuration that co ...
Unit B review - mvhs
... (A) A, B, and C will decrease. (B) A, B, and C will increase. (C) A will increase, B and C will decrease. (D) A and B will increase, C will decrease. (E) A will decrease, B and C will increase. 15. In any one period of the periodic table, the element in Group I, as compared to the element in Group V ...
... (A) A, B, and C will decrease. (B) A, B, and C will increase. (C) A will increase, B and C will decrease. (D) A and B will increase, C will decrease. (E) A will decrease, B and C will increase. 15. In any one period of the periodic table, the element in Group I, as compared to the element in Group V ...
CHEMISTRY ACTIVITY—MOLECULAR GEOMETRY Go to this
... Realize, then, that the 4 electron pairs around the central atom in H2O and in CH4 are not much different, except that some are unbonded (lone) in H2O. This accounts for the differences in shape and bond angle, since LONE PAIRS REPEL just like bonding pairs; in fact, they repel even more than bondin ...
... Realize, then, that the 4 electron pairs around the central atom in H2O and in CH4 are not much different, except that some are unbonded (lone) in H2O. This accounts for the differences in shape and bond angle, since LONE PAIRS REPEL just like bonding pairs; in fact, they repel even more than bondin ...
Chemistry Midterm Review 2006
... us to observe flame tests? Is energy released or absorbed when an electron falls from a higher energy level to a lower energy level? 8. What is the difference between a ground state and an excited state? 9. What is the lowest energy level? The lowest sublevel? 10. What is the maximum number of elect ...
... us to observe flame tests? Is energy released or absorbed when an electron falls from a higher energy level to a lower energy level? 8. What is the difference between a ground state and an excited state? 9. What is the lowest energy level? The lowest sublevel? 10. What is the maximum number of elect ...
study guide first semester chemistry
... 1. Write the balanced equation for the following: (include the state of each reactant and product) a. magnesium reacts with nitrogen to produce magnesium nitride. (3Mg(s) + N2(g) Mg3N2(s) b. silver nitrate reacts with copper to form copper(II) nitrate and silver. (2AgNO3(aq) + Cu Cu(NO3)2(aq) +2 ...
... 1. Write the balanced equation for the following: (include the state of each reactant and product) a. magnesium reacts with nitrogen to produce magnesium nitride. (3Mg(s) + N2(g) Mg3N2(s) b. silver nitrate reacts with copper to form copper(II) nitrate and silver. (2AgNO3(aq) + Cu Cu(NO3)2(aq) +2 ...
Chemistry Part 1
... Rule of eights – Atoms are considered stable when their outermost orbital has 8 electrons – The exception to this rule of eights is Shell 1, which can only hold 2 electrons ...
... Rule of eights – Atoms are considered stable when their outermost orbital has 8 electrons – The exception to this rule of eights is Shell 1, which can only hold 2 electrons ...
Chemistry - El Camino College
... and are called ______ or electrolytes 2. _________ Bonds are strong chemical bonds between atoms that result from the _______ of electrons in their outer orbitals. Molecules with covalent bonds are represented 2 ways: a. ___________ formulas in which each pair of shared electrons is represented by a ...
... and are called ______ or electrolytes 2. _________ Bonds are strong chemical bonds between atoms that result from the _______ of electrons in their outer orbitals. Molecules with covalent bonds are represented 2 ways: a. ___________ formulas in which each pair of shared electrons is represented by a ...
Safety - Wando High School
... b. 8.7300 c. 14.000 d. 0.00038098 3. Convert the following into scientific notation a. 1,500,000 b. .000336 4. Round these numbers to 4 significant digits a. 48.275687 b. 123.456 c. 0.00637893 d. 12.56157 5. What are the rules for using significant digits while adding/subtracting? While multiplying/ ...
... b. 8.7300 c. 14.000 d. 0.00038098 3. Convert the following into scientific notation a. 1,500,000 b. .000336 4. Round these numbers to 4 significant digits a. 48.275687 b. 123.456 c. 0.00637893 d. 12.56157 5. What are the rules for using significant digits while adding/subtracting? While multiplying/ ...
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... 46.A physical property of a Cu is that it is malleable. 47.A physical property of Se is that it has luster. 48.A physical property of Br is that it conducts electricity. 49.An ionic charge between a metal and a non metal has a net charge of zero 50.PbO2 is Plumbic Oxide 51.N2O5 is dinitrogen pentoxi ...
... 46.A physical property of a Cu is that it is malleable. 47.A physical property of Se is that it has luster. 48.A physical property of Br is that it conducts electricity. 49.An ionic charge between a metal and a non metal has a net charge of zero 50.PbO2 is Plumbic Oxide 51.N2O5 is dinitrogen pentoxi ...
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.)