Unit 6 Worksheet Package
... 6. Apply the octet rule to describe molecular structures. 7. List exceptions to the octet rule. 8. Define bond energies and explain how they can be used to compare bond strengths of different chemical bonds. 9. Describe polarity in bonds and how that can create hydrogen bonding. 10. Explain how a mo ...
... 6. Apply the octet rule to describe molecular structures. 7. List exceptions to the octet rule. 8. Define bond energies and explain how they can be used to compare bond strengths of different chemical bonds. 9. Describe polarity in bonds and how that can create hydrogen bonding. 10. Explain how a mo ...
chapter 2 - Scranton Prep Biology
... . An atom with a complete valence shell is unreactiveor inert' . Noble elements (e.g., helium, argon, and neon) have filled outer shells in their elemental state and are thus inert' . An atom with an incomplete valence shell is chemically reactive (tends to form chemical bonds uniil it has eight ele ...
... . An atom with a complete valence shell is unreactiveor inert' . Noble elements (e.g., helium, argon, and neon) have filled outer shells in their elemental state and are thus inert' . An atom with an incomplete valence shell is chemically reactive (tends to form chemical bonds uniil it has eight ele ...
Chem312 Au03 Problem Set 4
... of one electron from the t2g set of orbitals to the t2g eg set. In a diagram like the one at right, add ground state excited state electrons to represent the ground state and the lowest energy excited state. When you put the electrons in, you should follow Hund’s rule, that a state is lower in energ ...
... of one electron from the t2g set of orbitals to the t2g eg set. In a diagram like the one at right, add ground state excited state electrons to represent the ground state and the lowest energy excited state. When you put the electrons in, you should follow Hund’s rule, that a state is lower in energ ...
Review Sheet for Chemistry* First Semester Final
... What does an emission spectrum allow one to do? ...
... What does an emission spectrum allow one to do? ...
sample - Bright Red Publishing
... where HP and HR are the enthalpies of the products and reactants respectively. This expression tells us that ∆H could be calculated if we knew the actual enthalpies of all the reactants and products. However, there is no way we can determine the absolute value of the enthalpy of a substance. Only va ...
... where HP and HR are the enthalpies of the products and reactants respectively. This expression tells us that ∆H could be calculated if we knew the actual enthalpies of all the reactants and products. However, there is no way we can determine the absolute value of the enthalpy of a substance. Only va ...
Chapter Outline • Review of Atomic Structure Electrons, protons
... (non-metallic) atoms from the right that are happy to get one or a few electrons to acquire stable or noble gas electron configuration. As a result of this transfer mutual ionization occurs: atom that gives up electron(s) becomes positively charged ion (cation), atom that accepts electron(s) becomes ...
... (non-metallic) atoms from the right that are happy to get one or a few electrons to acquire stable or noble gas electron configuration. As a result of this transfer mutual ionization occurs: atom that gives up electron(s) becomes positively charged ion (cation), atom that accepts electron(s) becomes ...
Remember Question words
... shell = a particular region where electrons can orbit the nucleus of an atom valence electron = an electron in the outermost shell of an atom charges (positive = proton; neutral = neutron; negative = ...
... shell = a particular region where electrons can orbit the nucleus of an atom valence electron = an electron in the outermost shell of an atom charges (positive = proton; neutral = neutron; negative = ...
Original
... -2 electrons (1 from each separate hydrogen) are available for bonding -the energy of the electrons goes into the bonding molecular orbital and therefore is lower than the energy of the electrons in the atomic orbitals of separate hydrogen atoms -result is a stable covalent bond between the hydrogen ...
... -2 electrons (1 from each separate hydrogen) are available for bonding -the energy of the electrons goes into the bonding molecular orbital and therefore is lower than the energy of the electrons in the atomic orbitals of separate hydrogen atoms -result is a stable covalent bond between the hydrogen ...
Quiz 1 - sample quiz
... 9. Which one of the following statements is false? a) An electron jumps from a high energy orbital to a lower energy orbital when a photon of energy is emitted by an atom. b) The energy of light is directly proportional to its wavelength. c) The atomic emission spectrum consists of a series of discr ...
... 9. Which one of the following statements is false? a) An electron jumps from a high energy orbital to a lower energy orbital when a photon of energy is emitted by an atom. b) The energy of light is directly proportional to its wavelength. c) The atomic emission spectrum consists of a series of discr ...
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 ...
Electro-magnetic radiation (light)
... Energies of Orbitals • For a one-electron hydrogen atom, orbitals on the same energy level have the same energy. • That is, they are degenerate. ...
... Energies of Orbitals • For a one-electron hydrogen atom, orbitals on the same energy level have the same energy. • That is, they are degenerate. ...
File - Mr. Holz`s Website
... Ionic Bond – Transfer of electrons to create a bond between two ions that are attracted by opposite charges Covalent Bond – Bond that forms when electrons are shared between atoms Ion – Charged atoms that form from ionic bonds; atoms in which the number of electrons does not equal the number of prot ...
... Ionic Bond – Transfer of electrons to create a bond between two ions that are attracted by opposite charges Covalent Bond – Bond that forms when electrons are shared between atoms Ion – Charged atoms that form from ionic bonds; atoms in which the number of electrons does not equal the number of prot ...
Unit 16 Worksheet - Jensen Chemistry
... Name_________________________________________________period____________Unit 16: reaction rates Review: 1. When do electrons release photons(packets of energy)? When the electrons: a. move to higher levels of energy b. return to their original energy level c increase orbital speed around the nucleus ...
... Name_________________________________________________period____________Unit 16: reaction rates Review: 1. When do electrons release photons(packets of energy)? When the electrons: a. move to higher levels of energy b. return to their original energy level c increase orbital speed around the nucleus ...
Slide 1
... The symbol for the magnetic quantum number is m which defines the orbital. m = - , (- + 1), (- +2), .....0, ......., ( -2), ( -1), The last quantum number is the spin quantum number which has the symbol m s which characterizes the single electron. The spin quantum number only has two pos ...
... The symbol for the magnetic quantum number is m which defines the orbital. m = - , (- + 1), (- +2), .....0, ......., ( -2), ( -1), The last quantum number is the spin quantum number which has the symbol m s which characterizes the single electron. The spin quantum number only has two pos ...
Ch. 8 Sections 8.1-8.3 Powerpoint
... representative elements. •Range is from 4.0 for fluorine (most electronegative element) to 0.7 for cesium. ...
... representative elements. •Range is from 4.0 for fluorine (most electronegative element) to 0.7 for cesium. ...
unit 2 - chemistry
... 1. nucleus – p+ and n0 (inside) e- - (outside) 2. #e- = #p+ d. atomic number is the number of protons e. atomic mass =p+ + n0 f. electrons in energy levels – 2,8,18, etc… 1.electrons jump – light releases 2.atom – attempts to fill outer levels (valence) and bonding is the result 3.bonding – sharing, ...
... 1. nucleus – p+ and n0 (inside) e- - (outside) 2. #e- = #p+ d. atomic number is the number of protons e. atomic mass =p+ + n0 f. electrons in energy levels – 2,8,18, etc… 1.electrons jump – light releases 2.atom – attempts to fill outer levels (valence) and bonding is the result 3.bonding – sharing, ...
Semester Exam Review Guide
... 24. Plasmas include all of the following except: a. ionized gases b. lava c. lightning d. stars 26. If the mass of a steel bolt is 4.0 grams and its volume is 2 milliliters, what is the bolt’s density? a. 2 ml / g b. 2 g / ml c. .5 g / ml d. 8 ml / g 27. How many Hydrogen atoms are in the following ...
... 24. Plasmas include all of the following except: a. ionized gases b. lava c. lightning d. stars 26. If the mass of a steel bolt is 4.0 grams and its volume is 2 milliliters, what is the bolt’s density? a. 2 ml / g b. 2 g / ml c. .5 g / ml d. 8 ml / g 27. How many Hydrogen atoms are in the following ...
Molecular orbital diagram
A molecular orbital diagram, or MO diagram, is a qualitative descriptive tool explaining chemical bonding in molecules in terms of molecular orbital theory in general and the linear combination of atomic orbitals (LCAO) molecular orbital method in particular. A fundamental principle of these theories is that as atoms bond to form molecules, a certain number of atomic orbitals combine to form the same number of molecular orbitals, although the electrons involved may be redistributed among the orbitals. This tool is very well suited for simple diatomic molecules such as dihydrogen, dioxygen, and carbon monoxide but becomes more complex when discussing even comparatively simple polyatomic molecules, such as methane. MO diagrams can explain why some molecules exist and others do not. They can also predict bond strength, as well as the electronic transitions that can take place.