Biochemistry-Review of the Basics
... H-bonds are collectively strong so water can absorb much energy (heat) w/o a big temp change ...
... H-bonds are collectively strong so water can absorb much energy (heat) w/o a big temp change ...
Resource for Final Exam Prep
... H = q at constant pressure (open system such as coffee-cup calorimeter) E = q at constant volume (closed system such as bomb calorimeter) Hess’s Law of manipulating thermochemical equations Different energy units, fuel density, Food calorie etc Chapter-6: E = h and n = c/ So, E = hc/ 1 nm = 1 ...
... H = q at constant pressure (open system such as coffee-cup calorimeter) E = q at constant volume (closed system such as bomb calorimeter) Hess’s Law of manipulating thermochemical equations Different energy units, fuel density, Food calorie etc Chapter-6: E = h and n = c/ So, E = hc/ 1 nm = 1 ...
Atoms, Ions, and Molecules File
... The modern view of matter did not emerge until 1806 with John Dalton’s atomic theory: • Each element is composed of atoms. • Atoms of a given element are all the same. Atoms of different elements are different. • Atoms are not changed into different atoms in a chemical reaction. • Compounds are form ...
... The modern view of matter did not emerge until 1806 with John Dalton’s atomic theory: • Each element is composed of atoms. • Atoms of a given element are all the same. Atoms of different elements are different. • Atoms are not changed into different atoms in a chemical reaction. • Compounds are form ...
final exam practice test - Clayton State University
... b. The presence of lone (unshared) pairs of electrons affect the dipole moment of a molecule. c. Generally, as electronegativity differences increases in diatomic molecules, the dipole moments increase. d. The dipole moment equals the product of charge and distance of separation of the charges. e. B ...
... b. The presence of lone (unshared) pairs of electrons affect the dipole moment of a molecule. c. Generally, as electronegativity differences increases in diatomic molecules, the dipole moments increase. d. The dipole moment equals the product of charge and distance of separation of the charges. e. B ...
topic 3: periodicity
... in non-metallic elements: the atomic radius is half the distance between the centres of two covalently bonded atoms (= covalent radius). In table 8 of the data booklet, there is no atomic radius for inert gases as they do not make covalent bonds in diatomic molecules. in metallic elements: the a ...
... in non-metallic elements: the atomic radius is half the distance between the centres of two covalently bonded atoms (= covalent radius). In table 8 of the data booklet, there is no atomic radius for inert gases as they do not make covalent bonds in diatomic molecules. in metallic elements: the a ...
ch04_sec3_as - LCMR School District
... Bellringer In an atom, an energy level is an area around the nucleus where electrons are located. Each energy level may contain only a certain number of electrons. The electrons in an atom’s outer energy level are called valence electrons, which determine the chemical properties of an atom. The diag ...
... Bellringer In an atom, an energy level is an area around the nucleus where electrons are located. Each energy level may contain only a certain number of electrons. The electrons in an atom’s outer energy level are called valence electrons, which determine the chemical properties of an atom. The diag ...
Section 3: Modern Atomic Theory Atoms Section 3
... Bellringer In an atom, an energy level is an area around the nucleus where electrons are located. Each energy level may contain only a certain number of electrons. The electrons in an atom’s outer energy level are called valence electrons, which determine the chemical properties of an atom. The diag ...
... Bellringer In an atom, an energy level is an area around the nucleus where electrons are located. Each energy level may contain only a certain number of electrons. The electrons in an atom’s outer energy level are called valence electrons, which determine the chemical properties of an atom. The diag ...
AP Chem Test 5-7 Practice Exam - mvhs
... Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3CO2(g) ΔH = -28.0 kJ 3Fe(s) + 4 CO2(g) 4CO(g) + Fe3O4(s) ΔH = +12.5 kJ the enthalpy of the reaction of Fe2O3 with CO 3 Fe2O3(s) + CO(g) CO2(g) + 2 Fe3O4(s) is __________ kJ. A) -59.0 B) 40.5 C) -15.5 D) -109 E) +109 ...
... Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3CO2(g) ΔH = -28.0 kJ 3Fe(s) + 4 CO2(g) 4CO(g) + Fe3O4(s) ΔH = +12.5 kJ the enthalpy of the reaction of Fe2O3 with CO 3 Fe2O3(s) + CO(g) CO2(g) + 2 Fe3O4(s) is __________ kJ. A) -59.0 B) 40.5 C) -15.5 D) -109 E) +109 ...
Second Semester Notes 09-10
... 1.0 mole = 6.02 x 1023 atoms or molecules = ? g = 22.4 L (at STP) Percent Composition - the percentage by mass of each element in a compound ...
... 1.0 mole = 6.02 x 1023 atoms or molecules = ? g = 22.4 L (at STP) Percent Composition - the percentage by mass of each element in a compound ...
Document
... Atoms gain electrons (negatives) and become more negative. Atoms with 2-3 valence electrons will LOSE electrons and become more positive. Who will lose and who will gain an electron? ...
... Atoms gain electrons (negatives) and become more negative. Atoms with 2-3 valence electrons will LOSE electrons and become more positive. Who will lose and who will gain an electron? ...
Unit 1
... Bond between molecules NOT between atoms Results from a covalent bond involving hydrogen Shared electron spends more time around the bigger nucleus of the Oxygen atom This leaves the hydrogen end with a net positive charge & the Oxygen end with a net negative. A polar molecule due to the charge diff ...
... Bond between molecules NOT between atoms Results from a covalent bond involving hydrogen Shared electron spends more time around the bigger nucleus of the Oxygen atom This leaves the hydrogen end with a net positive charge & the Oxygen end with a net negative. A polar molecule due to the charge diff ...
Unit 1
... Bond between molecules NOT between atoms Results from a covalent bond involving hydrogen Shared electron spends more time around the bigger nucleus of the Oxygen atom This leaves the hydrogen end with a net positive charge & the Oxygen end with a net negative. A polar molecule due to the charge diff ...
... Bond between molecules NOT between atoms Results from a covalent bond involving hydrogen Shared electron spends more time around the bigger nucleus of the Oxygen atom This leaves the hydrogen end with a net positive charge & the Oxygen end with a net negative. A polar molecule due to the charge diff ...
The Egyptian American International School
... The Bohr model assumed electrons travel around the nucleus in circular orbits which is incorrect. Schrodinger’s wave mechanical model assumes the electron has both particle and wave properties and describes electrons as occupying orbitals. 1. The orbitals are different from the Bohr orbits. 2. P ...
... The Bohr model assumed electrons travel around the nucleus in circular orbits which is incorrect. Schrodinger’s wave mechanical model assumes the electron has both particle and wave properties and describes electrons as occupying orbitals. 1. The orbitals are different from the Bohr orbits. 2. P ...
Measuring and Calculating
... Naming – always name the ions not the formulas (cation then anion). Name tells the 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 ...
... Naming – always name the ions not the formulas (cation then anion). Name tells the 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 ...
Unit 3C Standards for Quiz
... It will be similar to the last exam but there will be at least three questions per standard. Remember that since no calculators are allowed on the standards exam that we will be modeling this in this assessment of progress. Atomic and Molecular Structure 1. The Periodic Table displays the elements i ...
... It will be similar to the last exam but there will be at least three questions per standard. Remember that since no calculators are allowed on the standards exam that we will be modeling this in this assessment of progress. Atomic and Molecular Structure 1. The Periodic Table displays the elements i ...
Chp 1,2 rev
... What is the electron configuration for Al? S? Give the Aufbau principle, Hund’s rule, and Pauli exclusion principle. ...
... What is the electron configuration for Al? S? Give the Aufbau principle, Hund’s rule, and Pauli exclusion principle. ...
Unit 1 – Physical Science and Chemical Reactions
... By releasing (+ve) alpha particles at a thin gold foil Rutherford was astonished that a small percentage were deflected at large angles. He suggested that the atom must have a small, dense, positively charged inner core called a nucleus. He called these positively charged particles inside the nu ...
... By releasing (+ve) alpha particles at a thin gold foil Rutherford was astonished that a small percentage were deflected at large angles. He suggested that the atom must have a small, dense, positively charged inner core called a nucleus. He called these positively charged particles inside the nu ...
S3 Chemistry - eduBuzz.org
... State that elements are listed in the periodic table in order of increasing atomic number State that some groups contain elements with similar chemical properties State the definition of an isotope Appreciate the varying stability and practical application of isotopes Describe the relation ...
... State that elements are listed in the periodic table in order of increasing atomic number State that some groups contain elements with similar chemical properties State the definition of an isotope Appreciate the varying stability and practical application of isotopes Describe the relation ...
Learning Outcomes for Chemical Reactions and
... • State that elements are listed in the periodic table in order of increasing atomic number • State that some groups contain elements with similar chemical properties • State the definition of an isotope • Appreciate the varying stability and practical application of isotopes • Describe the relation ...
... • State that elements are listed in the periodic table in order of increasing atomic number • State that some groups contain elements with similar chemical properties • State the definition of an isotope • Appreciate the varying stability and practical application of isotopes • Describe the relation ...
Earth Materials
... An element is a substance that can not be broken down into others by ordinary chemical reactions An atom is a chemical unit that cannot be broken down by chemical means composed of: • Protons (positively charged) • Neutrons (zero net charge) • Electrons (negatively charged) ...
... An element is a substance that can not be broken down into others by ordinary chemical reactions An atom is a chemical unit that cannot be broken down by chemical means composed of: • Protons (positively charged) • Neutrons (zero net charge) • Electrons (negatively charged) ...
Preview Sample 1
... ionic compounds. Covalent bonds are strong chemical bonds that occur when atoms share electrons. Methane and sugar are examples of covalent compounds. 2. What information can be obtained from the periodic table of elements? From the periodic table, an element's symbol, atomic number, number of proto ...
... ionic compounds. Covalent bonds are strong chemical bonds that occur when atoms share electrons. Methane and sugar are examples of covalent compounds. 2. What information can be obtained from the periodic table of elements? From the periodic table, an element's symbol, atomic number, number of proto ...
File
... Carried out in a Hoffman’s apparatus (shown to the right), it splits water compounds into oxygen molecules and hydrogen molecules Water Oxygen + Hydrogen H2O O2 +H2 The electrolysis reaction proves that compounds are made of more than one kind of element. Dalton’s Atomic Theory: 1. All matte ...
... Carried out in a Hoffman’s apparatus (shown to the right), it splits water compounds into oxygen molecules and hydrogen molecules Water Oxygen + Hydrogen H2O O2 +H2 The electrolysis reaction proves that compounds are made of more than one kind of element. Dalton’s Atomic Theory: 1. All matte ...
Chapter 2 Study Guides
... 7. Before a chemical reaction can start, ____________________ must be absorbed by the reactants. The amount that must be absorbed to start the reaction is called the ...
... 7. Before a chemical reaction can start, ____________________ must be absorbed by the reactants. The amount that must be absorbed to start the reaction is called the ...
Family
... Electrons – Have a negative (-) charge and are located outside of the nucleus. Electrons are very small and move very fast making their location difficult to pin point. The general area where they are located is called an electron cloud or orbital. ...
... Electrons – Have a negative (-) charge and are located outside of the nucleus. Electrons are very small and move very fast making their location difficult to pin point. The general area where they are located is called an electron cloud or orbital. ...
Matter—anything that has mass and occupies space Weight—pull of
... Unequal sharing of electrons produces polar (AKA dipole) molecules such as H2O Atoms in bond have different electron-attracting abilities Small atoms with six or seven valence shell electrons are electronegative, e.g., oxygen Strong electron-attracting ability Most atoms with one or two valence shel ...
... Unequal sharing of electrons produces polar (AKA dipole) molecules such as H2O Atoms in bond have different electron-attracting abilities Small atoms with six or seven valence shell electrons are electronegative, e.g., oxygen Strong electron-attracting ability Most atoms with one or two valence shel ...
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.)