Chem Unit 2 Review Guide ANSWERS
... Conservation of Mass apply to each type of reaction? Chemical reactions only involve the atoms’ valence electrons. In a nuclear reaction, the nucleus is actually altered. The Law of Conservation of Mass holds true during chemical reactions, but is not during a nuclear reaction, as mass is converted ...
... Conservation of Mass apply to each type of reaction? Chemical reactions only involve the atoms’ valence electrons. In a nuclear reaction, the nucleus is actually altered. The Law of Conservation of Mass holds true during chemical reactions, but is not during a nuclear reaction, as mass is converted ...
Review for Exam 1
... Determine how many of each ion type is needed for an overall charge of zero. When the cation and anion have different charges, use the ion charges to determine the number of ions of each needed. ...
... Determine how many of each ion type is needed for an overall charge of zero. When the cation and anion have different charges, use the ion charges to determine the number of ions of each needed. ...
Atomic Structure 1. Historical perspective of the model of the atom a
... a.) In 1803, John Dalton proposed the atomic theory which stated that all matter is made of atoms, atoms of the same type of element have the same chemical properties, compounds are formed by two or more different types of atoms, and that a chemical reaction involves either, joining, separating, or ...
... a.) In 1803, John Dalton proposed the atomic theory which stated that all matter is made of atoms, atoms of the same type of element have the same chemical properties, compounds are formed by two or more different types of atoms, and that a chemical reaction involves either, joining, separating, or ...
Atomic Structure, Molecular Structure & Bonding
... 4. Count ve-’s and compare to #2 5. If too many e-’s, make a double bond 6. Calculate formal charge (FC) to double check structure – No or low FCs (e.g. +1) more likely than large FCs (e.g. ...
... 4. Count ve-’s and compare to #2 5. If too many e-’s, make a double bond 6. Calculate formal charge (FC) to double check structure – No or low FCs (e.g. +1) more likely than large FCs (e.g. ...
Covalent bonding
... Electronegativity & bond polarity Use the difference in electronegativity between atoms to gauge the polarity of a bond ...
... Electronegativity & bond polarity Use the difference in electronegativity between atoms to gauge the polarity of a bond ...
2 ppt
... Polar covalent bonds Pair of electrons not shared equally by 2 atoms Water = O + H oxygen has stronger “attraction” for the shared electrons than hydrogen oxygen has higher electronegativity ...
... Polar covalent bonds Pair of electrons not shared equally by 2 atoms Water = O + H oxygen has stronger “attraction” for the shared electrons than hydrogen oxygen has higher electronegativity ...
VOCABULARY name, date, hour: Fill in the number of each term
... ___ substance that is a mixture of two or more metals ___ columns of the periodic table; also known as groups ___ number of protons carried by the nucleus of an atom ___ element with an imbalance in the number of neutrons and protons ___ uncharged particle found in the nucleus of an atom ___ physica ...
... ___ substance that is a mixture of two or more metals ___ columns of the periodic table; also known as groups ___ number of protons carried by the nucleus of an atom ___ element with an imbalance in the number of neutrons and protons ___ uncharged particle found in the nucleus of an atom ___ physica ...
Notes
... -the number of protons in an atom of an element •all atoms of an element have the same atomic # •written as a subscript next to the element’s symbol •in a neutral atom, the number of protons is equal to the number of electrons (balanced charges). ...
... -the number of protons in an atom of an element •all atoms of an element have the same atomic # •written as a subscript next to the element’s symbol •in a neutral atom, the number of protons is equal to the number of electrons (balanced charges). ...
ATOMS
... • Most matter is in the form of COMPOUNDS or mixtures of compounds. For example: salt (NaCl), water (H20), carbon dioxide (CO2) • Compounds have properties UNLIKE those of their elements. For example: Salt—Sodium (Na) is a shiny, soft, gray, explosive metal with water & Chlorine (Cl) is a yellowish- ...
... • Most matter is in the form of COMPOUNDS or mixtures of compounds. For example: salt (NaCl), water (H20), carbon dioxide (CO2) • Compounds have properties UNLIKE those of their elements. For example: Salt—Sodium (Na) is a shiny, soft, gray, explosive metal with water & Chlorine (Cl) is a yellowish- ...
Pure Substances and Mixtures
... number of valence electrons can be determined by the column number; 1A has 1 valence electron, IIA has 2 valence electrons, etc. ...
... number of valence electrons can be determined by the column number; 1A has 1 valence electron, IIA has 2 valence electrons, etc. ...
Chemical Bond – a force that holds two atoms together, the bond
... Metallic Bond – is the attraction of a metallic cation for delocalized electrons; electrons are not localized to one metallic atom. Delocalized Electrons – electrons that freely move from one metallic atom to another metallic atom. Covalent Bond – a chemical bond between two different atomic elemen ...
... Metallic Bond – is the attraction of a metallic cation for delocalized electrons; electrons are not localized to one metallic atom. Delocalized Electrons – electrons that freely move from one metallic atom to another metallic atom. Covalent Bond – a chemical bond between two different atomic elemen ...
Science Olympiad
... (B) atomic radius decreases due to an increase in effective nuclear charge. (C) electronegativity decreases due to an increase in atomic radius. (D) electron affinity decreases due to an increase in effective nuclear charge. (E) ionization energy increases due to an increase in atomic radius. ______ ...
... (B) atomic radius decreases due to an increase in effective nuclear charge. (C) electronegativity decreases due to an increase in atomic radius. (D) electron affinity decreases due to an increase in effective nuclear charge. (E) ionization energy increases due to an increase in atomic radius. ______ ...
Chemistry Unit Study Guide Key
... or more elements that are bonded together; An element is a pure, single substance made of one type of atom. 2) examples of compounds – CO2, C6H12O6, NaCl, N2, O2, Fe2O3, H2O 3) where metals and nonmetals are found on the periodic table – Metals are to the left of the zig-zag line; Non-metals are to ...
... or more elements that are bonded together; An element is a pure, single substance made of one type of atom. 2) examples of compounds – CO2, C6H12O6, NaCl, N2, O2, Fe2O3, H2O 3) where metals and nonmetals are found on the periodic table – Metals are to the left of the zig-zag line; Non-metals are to ...
Small Business Success on the Web
... 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) ...
SEMESTER 1 EXAM Prblms/Short Ans
... 16.Write the formulas for the following binary compounds formed between the following elements: (#1 p. 223) a. Sodium and sulfur _______________________ d. aluminum and nitrogen __________________ Name the binary ionic compound as indicated by the following formulas: (#2 p. 223) b. AgCl ___________ ...
... 16.Write the formulas for the following binary compounds formed between the following elements: (#1 p. 223) a. Sodium and sulfur _______________________ d. aluminum and nitrogen __________________ Name the binary ionic compound as indicated by the following formulas: (#2 p. 223) b. AgCl ___________ ...
atoms, molecules, and matter (2)
... All earthly objects are a mixture of: 1. EARTH (bottom – center of universe) 2. WATER (water covers earth) 3. AIR (air over water) 4. FIRE (highest – at top) 5. Ether = QUINTESSENCE (Latin) – substance whose natural motion is that most symmetrical and eternal of all conceivable motion = endless circ ...
... All earthly objects are a mixture of: 1. EARTH (bottom – center of universe) 2. WATER (water covers earth) 3. AIR (air over water) 4. FIRE (highest – at top) 5. Ether = QUINTESSENCE (Latin) – substance whose natural motion is that most symmetrical and eternal of all conceivable motion = endless circ ...
05 Chemistry Basics with Flips 2011
... 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) ...
Midterm Review
... • Compared to the charge and mass of a proton, an electron has: 1. the same charge and a smaller mass 2. the same charge and the same mass 3. an opposite charge and a smaller mass 4. an opposite charge and the same mass ...
... • Compared to the charge and mass of a proton, an electron has: 1. the same charge and a smaller mass 2. the same charge and the same mass 3. an opposite charge and a smaller mass 4. an opposite charge and the same mass ...
Chapter 2 - Chemical Context of Life
... Mass number (Atomic mass) = p+ + n0 Isotopes are the different forms of an element. ...
... Mass number (Atomic mass) = p+ + n0 Isotopes are the different forms of an element. ...
Chemical Compounds
... S Take your ion and find someone you can bond with S Attempt to create the compound H2O, MgCl2..and so on S We will come together as a class and try to figure out if you ...
... S Take your ion and find someone you can bond with S Attempt to create the compound H2O, MgCl2..and so on S We will come together as a class and try to figure out if you ...
Chapter 2 BIO 100 Chemistry
... • Electrons = Negatively (-) charged particles that orbit around the nucleus. ...
... • Electrons = Negatively (-) charged particles that orbit around the nucleus. ...
6.1 Organizing the Periodic Table
... • Arranged the elements into rows in order of increasing mass so that elements with similar properties were in the same column • Left empty spaces where undiscovered elements would fit ...
... • Arranged the elements into rows in order of increasing mass so that elements with similar properties were in the same column • Left empty spaces where undiscovered elements would fit ...
1 - M*W
... d) Have the same number of electrons 23) To draw a Lewis structure you do not need to know a) The number of valence electrons for each atom b) The types of atoms in the molecule c) The number of atoms in the molecule d) Bond energies 24) Neils Bohr’s contribution to modern atomic theory was the prop ...
... d) Have the same number of electrons 23) To draw a Lewis structure you do not need to know a) The number of valence electrons for each atom b) The types of atoms in the molecule c) The number of atoms in the molecule d) Bond energies 24) Neils Bohr’s contribution to modern atomic theory was the prop ...
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.)