bonding, structure, properties and energy changes
... If heat energy is absorbed during a reaction, the temperature of the surroundings decreases and the reaction is described as being endothermic. When methylated spirits (‘meths’) is spilt on the skin it quickly evaporates. This is an endothermic process – the meths absorbs heat energy from the skin a ...
... If heat energy is absorbed during a reaction, the temperature of the surroundings decreases and the reaction is described as being endothermic. When methylated spirits (‘meths’) is spilt on the skin it quickly evaporates. This is an endothermic process – the meths absorbs heat energy from the skin a ...
Sections 6.4 - 6.5
... Inert Pair effect: Although the ionization energy decreases down the group with increasing atomic radius (heavier elements form cations more readily), the heavier elements also show greater stability of M+ (ns2np0). One possible explanation is that the ns2 electrons are harder to remove due to a rel ...
... Inert Pair effect: Although the ionization energy decreases down the group with increasing atomic radius (heavier elements form cations more readily), the heavier elements also show greater stability of M+ (ns2np0). One possible explanation is that the ns2 electrons are harder to remove due to a rel ...
CHEMISTRY I Final..#1..rev 4KEY
... Objective 2.07: Assess covalent bonding in molecular compounds as related to chemical and physical properties and molecular geometry. 38. The boiling point of HBr is lower than that of HF because: a. HBr is heavier than HF and therefore it requires less energy to vaporize. b. HBr has dipole-dipole ...
... Objective 2.07: Assess covalent bonding in molecular compounds as related to chemical and physical properties and molecular geometry. 38. The boiling point of HBr is lower than that of HF because: a. HBr is heavier than HF and therefore it requires less energy to vaporize. b. HBr has dipole-dipole ...
Chemical Nomenclature (ionic compounds)
... Scientists have agreed on a set of rules that govern the naming and formulation of compounds. It is universal! The following pages are a programmed approach to the problem of obtaining either the formula or name of a chemical compound. a) The compound will be formed by combining a metal and a non-me ...
... Scientists have agreed on a set of rules that govern the naming and formulation of compounds. It is universal! The following pages are a programmed approach to the problem of obtaining either the formula or name of a chemical compound. a) The compound will be formed by combining a metal and a non-me ...
200things2know
... Which of the following atoms forms a stable ion that does not have an octet structure? Li F Na Cl 98. Covalent bonds form when two atoms share a pair of electrons. How many covalent bonds are found in a nitrogen (N2) molecule? 99. Ionic bonds form when one atom transfers an electron to another atom ...
... Which of the following atoms forms a stable ion that does not have an octet structure? Li F Na Cl 98. Covalent bonds form when two atoms share a pair of electrons. How many covalent bonds are found in a nitrogen (N2) molecule? 99. Ionic bonds form when one atom transfers an electron to another atom ...
Midterm Review Answers
... 41. Which of the following sets of quantum numbers (n, l, ml, ms) best describes the valence electron of highest energy in a ground-state gallium atom (atomic number 31) ? (D) 4, 1, 2, 1/2 (E) 4, 2, 0, 1/2 ...
... 41. Which of the following sets of quantum numbers (n, l, ml, ms) best describes the valence electron of highest energy in a ground-state gallium atom (atomic number 31) ? (D) 4, 1, 2, 1/2 (E) 4, 2, 0, 1/2 ...
200 Ways to Pass the Chemistry
... Which of the following atoms forms a stable ion that does not have an octet structure? Li F Na Cl 98. Covalent bonds form when two atoms share a pair of electrons. How many covalent bonds are found in a nitrogen (N2) molecule? 99. Ionic bonds form when one atom transfers an electron to another atom ...
... Which of the following atoms forms a stable ion that does not have an octet structure? Li F Na Cl 98. Covalent bonds form when two atoms share a pair of electrons. How many covalent bonds are found in a nitrogen (N2) molecule? 99. Ionic bonds form when one atom transfers an electron to another atom ...
200 Things to Know to Pass the Chemistry Regents
... Which of the following atoms forms a stable ion that does not have an octet structure? Li F Na Cl 98. Covalent bonds form when two atoms share a pair of electrons. How many covalent bonds are found in a nitrogen (N2) molecule? 99. Ionic bonds form when one atom transfers an electron to another atom ...
... Which of the following atoms forms a stable ion that does not have an octet structure? Li F Na Cl 98. Covalent bonds form when two atoms share a pair of electrons. How many covalent bonds are found in a nitrogen (N2) molecule? 99. Ionic bonds form when one atom transfers an electron to another atom ...
Chemistry Standard Course of Study -- Detailed - UNCG GK-12
... 2.07 Assess covalent bonding in molecular compounds as related to molecular geometry and chemical and physical properties. ...
... 2.07 Assess covalent bonding in molecular compounds as related to molecular geometry and chemical and physical properties. ...
Radioactive Reactions
... Chemical Reaction • All chemical reactions involve the movement of valence electron in which chemical bonds are formed • Atoms want to have a stable outer energy level. • Valence electrons move in a way that stabilizes the atom outer energy level. – Ionic bond: one atom gives the other receives an ...
... Chemical Reaction • All chemical reactions involve the movement of valence electron in which chemical bonds are formed • Atoms want to have a stable outer energy level. • Valence electrons move in a way that stabilizes the atom outer energy level. – Ionic bond: one atom gives the other receives an ...
Biol 1406 notes Ch 2 8thed
... biological molecules it generally has a valence of 5, forming three single covalent bonds and one double bond. Covalent bonds can form between atoms of the same element or atoms of different elements. o Although both types are molecules, the latter are also compounds. o Water (H2O) is a compound in ...
... biological molecules it generally has a valence of 5, forming three single covalent bonds and one double bond. Covalent bonds can form between atoms of the same element or atoms of different elements. o Although both types are molecules, the latter are also compounds. o Water (H2O) is a compound in ...
Chapter 2
... Hydrogen bonds form when a hydrogen atom that is already covalently bonded to one electronegative atom is attracted to another electronegative atom. o In cells, the electronegative partners are typically nitrogen or oxygen. o Hydrogen bonds form because a polar covalent bond leaves the hydrogen atom ...
... Hydrogen bonds form when a hydrogen atom that is already covalently bonded to one electronegative atom is attracted to another electronegative atom. o In cells, the electronegative partners are typically nitrogen or oxygen. o Hydrogen bonds form because a polar covalent bond leaves the hydrogen atom ...
ch-4-earth-chemistry
... different number of neutrons or atomic mass would not change the atom into a different element. It just changes the atomic mass. ...
... different number of neutrons or atomic mass would not change the atom into a different element. It just changes the atomic mass. ...
Gr 10 Review sheet chemistry
... 1. Change of________________ 2. Formation of a ________________ 3. Formation of _____________ 4. Release or absorption of_____________ ...
... 1. Change of________________ 2. Formation of a ________________ 3. Formation of _____________ 4. Release or absorption of_____________ ...
Chemistry B2A Chapter 18 Oxidation
... Oxidation is the gain of oxygen atoms and/or the loss of hydrogen atoms. Reduction is the loss of oxygen atoms and/or the gain of hydrogen atoms. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) Therefore, CH4 is the reducing agent and O2 is the oxidizing agent. Note: When the oxidizing or reducing agent is named ...
... Oxidation is the gain of oxygen atoms and/or the loss of hydrogen atoms. Reduction is the loss of oxygen atoms and/or the gain of hydrogen atoms. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) Therefore, CH4 is the reducing agent and O2 is the oxidizing agent. Note: When the oxidizing or reducing agent is named ...
2012 Coaches Institute Presentation
... } Pauli Exclusion Principle – No more than 2 electrons in an orbital, one is spin up, the other spin down. } Hund s Rule – If 2 or more orbitals have the same energy, one electron goes in each until all are half full. Then, electrons go back and pair up. ...
... } Pauli Exclusion Principle – No more than 2 electrons in an orbital, one is spin up, the other spin down. } Hund s Rule – If 2 or more orbitals have the same energy, one electron goes in each until all are half full. Then, electrons go back and pair up. ...
Chemistry Reference Table Review
... 100 grams of H2O at 50°C is best described as (1) saturated and dilute (2) saturated and concentrated (3) supersaturated and dilute (4) supersaturated and concentrated 85. A student calculated the percent by mass of water in a sample of BaCl2 •2 H2O to be 16.4%, but the accepted value is 14.8%. What ...
... 100 grams of H2O at 50°C is best described as (1) saturated and dilute (2) saturated and concentrated (3) supersaturated and dilute (4) supersaturated and concentrated 85. A student calculated the percent by mass of water in a sample of BaCl2 •2 H2O to be 16.4%, but the accepted value is 14.8%. What ...
Chemistry 1 Revision: Metals and their uses
... nucleus periodic table properties protons right second shell sodium stable unreactive water +1 ...
... nucleus periodic table properties protons right second shell sodium stable unreactive water +1 ...
The Periodic table
... A region of space within an electron subshell where an electron with a specific energy is most likely to be found. S subshell=1 orbital, p subshell=3 orbitals, d subshell=5 orbitals, f subshell=7 orbitals. Maximum number of electrons in a subshell is always 2. S orbital=spherical, p orbital ...
... A region of space within an electron subshell where an electron with a specific energy is most likely to be found. S subshell=1 orbital, p subshell=3 orbitals, d subshell=5 orbitals, f subshell=7 orbitals. Maximum number of electrons in a subshell is always 2. S orbital=spherical, p orbital ...
honors chem 6 day review packet
... Metals _____________ electrons. They form __________________. Nonmetals ______________________ electrons. They form __________. Trends Atomic radius (size) ionization energy (energy to remove an electron) Electronegativity (ability to gain an electron) Reactivity for metal (metallic character) React ...
... Metals _____________ electrons. They form __________________. Nonmetals ______________________ electrons. They form __________. Trends Atomic radius (size) ionization energy (energy to remove an electron) Electronegativity (ability to gain an electron) Reactivity for metal (metallic character) React ...
Ei otsikkoa
... Chlorides are compounds of chlorine and one other element. Metal chlorides are ionic and thereby conduct electricity when molten or aqueous and have high melting points. Aluminium chloride, however, possesses a covalent ...
... Chlorides are compounds of chlorine and one other element. Metal chlorides are ionic and thereby conduct electricity when molten or aqueous and have high melting points. Aluminium chloride, however, possesses a covalent ...
Medical Physics and Statistics
... itself in a covalent bond. Sum of ionization energy and electron affinity. [Linus Pauling (1901-1994), Nobel Prize (1954 chemistry, 1962 peace)] ...
... itself in a covalent bond. Sum of ionization energy and electron affinity. [Linus Pauling (1901-1994), Nobel Prize (1954 chemistry, 1962 peace)] ...
Summer Work
... 5. No two different elements will have the ______________________ atomic number. 6. The ______________________ of an element is the average mass of an element’s naturally occurring atom, or isotopes, taking into account the ______________________ of each isotope. 7. The ______________________ of an ...
... 5. No two different elements will have the ______________________ atomic number. 6. The ______________________ of an element is the average mass of an element’s naturally occurring atom, or isotopes, taking into account the ______________________ of each isotope. 7. The ______________________ of an ...
High School Physical Science Glossary
... certain frequencies is absorbed acceleration- the change in velocity divided by time (a = Δv / Δt) accuracy- values such as density of a specific element that are accepted norms and usually published; if a measurement taken matches accepted norms or a standard value, it is said to be accurate acid/b ...
... certain frequencies is absorbed acceleration- the change in velocity divided by time (a = Δv / Δt) accuracy- values such as density of a specific element that are accepted norms and usually published; if a measurement taken matches accepted norms or a standard value, it is said to be accurate acid/b ...
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.)