Final exam 2007
... Name (last name first): _____________________________________________ I.D. Number last 4: _________________________________________________ Note: There are 18 questions in this exam. Fill in your answer in the blank space provided immediately following each question. 1/2 point will be subtracted eve ...
... Name (last name first): _____________________________________________ I.D. Number last 4: _________________________________________________ Note: There are 18 questions in this exam. Fill in your answer in the blank space provided immediately following each question. 1/2 point will be subtracted eve ...
Terminology 1
... Shows which elements are present and the simplest whole number ratio of their atoms, but not necessarily the actual number of atoms present in the molecule. (simplest chemical ...
... Shows which elements are present and the simplest whole number ratio of their atoms, but not necessarily the actual number of atoms present in the molecule. (simplest chemical ...
Lab Science 9 Pacing Guide
... the number of protons (called the atomic number), the repeating patterns of physical and chemical properties identify families of elements. Recognize that the periodic table was formed as a result of the repeating pattern of electron configurations. 5. Describe how ions are formed when an atom or a ...
... the number of protons (called the atomic number), the repeating patterns of physical and chemical properties identify families of elements. Recognize that the periodic table was formed as a result of the repeating pattern of electron configurations. 5. Describe how ions are formed when an atom or a ...
Trends in the Periodic Table
... – Largest atomic radius in the period • Very chemically reactive – One valence electron, easily lost, + ion • Tarnish quickly • Combine with O, Cl, Br to form ionic compounds ...
... – Largest atomic radius in the period • Very chemically reactive – One valence electron, easily lost, + ion • Tarnish quickly • Combine with O, Cl, Br to form ionic compounds ...
No Slide Title - Rubin Gulaboski
... • Rutherford assumed the electrons orbited the nucleus analogous to planets around the sun. • However, a charged particle moving in a circular path should lose energy. • This means that the atom should be unstable according to Rutherford’s theory. • Bohr noted the line spectra of certain elements an ...
... • Rutherford assumed the electrons orbited the nucleus analogous to planets around the sun. • However, a charged particle moving in a circular path should lose energy. • This means that the atom should be unstable according to Rutherford’s theory. • Bohr noted the line spectra of certain elements an ...
lewis dot diagrams (structures) for atoms and ions predicting
... Indicate whether the following statements are true (T) or false (F). If the statement is false, rewrite the statement to make it true. 1. Chemical bonding is the process of atoms combining to form new substances. 2. Valence electrons are in the innermost energy level. 3. Matter in its lowest energy ...
... Indicate whether the following statements are true (T) or false (F). If the statement is false, rewrite the statement to make it true. 1. Chemical bonding is the process of atoms combining to form new substances. 2. Valence electrons are in the innermost energy level. 3. Matter in its lowest energy ...
Keble College - Hilary 2012 1 Chemical bonding
... a particle is proportional to the inverse square of the size of a box containing it), and this underlies both covalent and metallic bonding. However, it is difficult to quantify the energy reduction due to delocalisation. To get a feel for the effect, we now study a toy model that captures the essen ...
... a particle is proportional to the inverse square of the size of a box containing it), and this underlies both covalent and metallic bonding. However, it is difficult to quantify the energy reduction due to delocalisation. To get a feel for the effect, we now study a toy model that captures the essen ...
Atoms, electrons, nuclei J.J. Thomson discovered the electron (1897
... through a thin metal foil: interference interference phenomena have been shown with various other particles: duality is a general characteristic of matter Propagation law of free electrons state function ψ(x,t); we can ‘find’ the electron where ψ(x,t) ≠ 0, its momentum p = mv is given by the ‘shape’ ...
... through a thin metal foil: interference interference phenomena have been shown with various other particles: duality is a general characteristic of matter Propagation law of free electrons state function ψ(x,t); we can ‘find’ the electron where ψ(x,t) ≠ 0, its momentum p = mv is given by the ‘shape’ ...
Advanced Chemistry Midterm
... 73. The relationship in which the physical and chemical properties of elements show a periodic pattern when the elements are arranged by increasing atomic number is called a. the periodic law b. the law of octaves c. Mendeleev’s law d. Meyer’s periodicity 74. The elements in group 1 (1A) of the peri ...
... 73. The relationship in which the physical and chemical properties of elements show a periodic pattern when the elements are arranged by increasing atomic number is called a. the periodic law b. the law of octaves c. Mendeleev’s law d. Meyer’s periodicity 74. The elements in group 1 (1A) of the peri ...
Chemistry 4021/8021 Computational Chemistry 3/4 Credits Spring
... combination of CN π bonds with a weak antibonding interaction with Ni, and orbital 42 is a symmetric combination of CO π* antibonds with no significant Ni contribution (only a Ni pz orbital would have the right phase behavior to participate in this orbital, and no such orbital is nearby in energy). ...
... combination of CN π bonds with a weak antibonding interaction with Ni, and orbital 42 is a symmetric combination of CO π* antibonds with no significant Ni contribution (only a Ni pz orbital would have the right phase behavior to participate in this orbital, and no such orbital is nearby in energy). ...
mp2b-16 honors
... Be able to write electron configurations and orbital filling diagrams a. What are the two types of electrons in an atom? Where are they? How do we define the outer electrons? a. Core style – short form b. Full style c. Orbital filling diagrams [show the arrows] d. Remember the exceptions in the firs ...
... Be able to write electron configurations and orbital filling diagrams a. What are the two types of electrons in an atom? Where are they? How do we define the outer electrons? a. Core style – short form b. Full style c. Orbital filling diagrams [show the arrows] d. Remember the exceptions in the firs ...
Molecular Geometry and Polarity - Clewett
... If the central atom does not have an octet, use >>> Only the second period elements C, N, O and lone pairs from terminal atoms to form multiple sometimes S (in combination with C or O) form multibonds. ple bonds. This leads to another exception to the octet rule, i.e. when an atom like Be is combine ...
... If the central atom does not have an octet, use >>> Only the second period elements C, N, O and lone pairs from terminal atoms to form multiple sometimes S (in combination with C or O) form multibonds. ple bonds. This leads to another exception to the octet rule, i.e. when an atom like Be is combine ...
1.3.4 Atoms and molecules Name Symbol Definition SI unit Notes
... The concept of electronegativity was intoduced by L. Pauling as the power of an atom in a molecule to attract electrons to itself. There are several ways of defining this quantity. The one given in the table has a clear physical meaning of energy and is due to R.S. Mulliken. The most frequently used ...
... The concept of electronegativity was intoduced by L. Pauling as the power of an atom in a molecule to attract electrons to itself. There are several ways of defining this quantity. The one given in the table has a clear physical meaning of energy and is due to R.S. Mulliken. The most frequently used ...
Chemistry Final Exam Review 2006-2007
... 21. What is the difference between the Bohr model and the Quantum mechanical model? 22. a. What are flame tests? b. What area of the electromagnetic radiation spectrum allows us to observe flame tests? c. Is energy released or absorbed when an electron falls from a higher energy level to a lower ene ...
... 21. What is the difference between the Bohr model and the Quantum mechanical model? 22. a. What are flame tests? b. What area of the electromagnetic radiation spectrum allows us to observe flame tests? c. Is energy released or absorbed when an electron falls from a higher energy level to a lower ene ...
Atomic Structure and Chemical Bonding
... Ans2. Lyman series: When excited electrons in hydrogen atoms fall from higher energy levels to first energy level, the series of lines observed are called Lyman series. They are observed in ultraviolet region. Lyman = R(1/12 - 1/n2), n = 2, 3, 4, 5, ......... Balmer series: When excited electrons in ...
... Ans2. Lyman series: When excited electrons in hydrogen atoms fall from higher energy levels to first energy level, the series of lines observed are called Lyman series. They are observed in ultraviolet region. Lyman = R(1/12 - 1/n2), n = 2, 3, 4, 5, ......... Balmer series: When excited electrons in ...
Lesson 1 - Working With Chemicals
... - protons are heavy positive particles within the nucleus o Electrons – particles with a negative charge and are very light (compared to protons). - Electrons circle around the nucleus o Empty space surrounding the nucleus is very large within which electrons move (planetary model). o Rutherford als ...
... - protons are heavy positive particles within the nucleus o Electrons – particles with a negative charge and are very light (compared to protons). - Electrons circle around the nucleus o Empty space surrounding the nucleus is very large within which electrons move (planetary model). o Rutherford als ...
Topic 2
... Atomic Theory of Matter – An element is a substance whose atoms all have the same atomic number (Z). The #protons defines the identity of an atom and can be found on the periodic table (large number in top of element box). – The neutron is a nuclear particle having a mass almost identical to that o ...
... Atomic Theory of Matter – An element is a substance whose atoms all have the same atomic number (Z). The #protons defines the identity of an atom and can be found on the periodic table (large number in top of element box). – The neutron is a nuclear particle having a mass almost identical to that o ...
The Periodic Table
... the core of an atom, called the nucleus The number of protons and neutrons add together to give the mass of the atom – each is designated a mass of 1 amu ...
... the core of an atom, called the nucleus The number of protons and neutrons add together to give the mass of the atom – each is designated a mass of 1 amu ...
CP Chemistry Final Exam Review Sheet
... 50. What is the octet rule? The octet rule states that atoms will gain, lose, or share electrons in order to get a full octet (8 e-) in the valence (outermost) shell of an atom. 51. An ion is a particle with an electrical charge created by the transfer (loss or gaining) of electrons. 52. What is a c ...
... 50. What is the octet rule? The octet rule states that atoms will gain, lose, or share electrons in order to get a full octet (8 e-) in the valence (outermost) shell of an atom. 51. An ion is a particle with an electrical charge created by the transfer (loss or gaining) of electrons. 52. What is a c ...
Practice Exam 3 - University of Missouri
... 7. The thermochemical equation which defines the enthalpy of formation of acetylene, C2H2(g) is a. 2 C(s) + H2(g) → C2H2(g) b. 2 C(g) + 2H(g) → C2H2(g) c. 2 C2(g) + 2H(g) → C2H2(g) d. C2H6(g) → C2H2(g) + H2 e. none of the above 8. Which of the following has a standard molar enthalpy of formation of ...
... 7. The thermochemical equation which defines the enthalpy of formation of acetylene, C2H2(g) is a. 2 C(s) + H2(g) → C2H2(g) b. 2 C(g) + 2H(g) → C2H2(g) c. 2 C2(g) + 2H(g) → C2H2(g) d. C2H6(g) → C2H2(g) + H2 e. none of the above 8. Which of the following has a standard molar enthalpy of formation of ...
Chemical bond
A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges, either between electrons and nuclei, or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are ""strong bonds"" such as covalent or ionic bonds and ""weak bonds"" such as Dipole-dipole interaction, the London dispersion force and hydrogen bonding.Since opposite charges attract via a simple electromagnetic force, the negatively charged electrons that are orbiting the nucleus and the positively charged protons in the nucleus attract each other. An electron positioned between two nuclei will be attracted to both of them, and the nuclei will be attracted toward electrons in this position. This attraction constitutes the chemical bond. Due to the matter wave nature of electrons and their smaller mass, they must occupy a much larger amount of volume compared with the nuclei, and this volume occupied by the electrons keeps the atomic nuclei relatively far apart, as compared with the size of the nuclei themselves. This phenomenon limits the distance between nuclei and atoms in a bond.In general, strong chemical bonding is associated with the sharing or transfer of electrons between the participating atoms. The atoms in molecules, crystals, metals and diatomic gases—indeed most of the physical environment around us—are held together by chemical bonds, which dictate the structure and the bulk properties of matter.All bonds can be explained by quantum theory, but, in practice, simplification rules allow chemists to predict the strength, directionality, and polarity of bonds. The octet rule and VSEPR theory are two examples. More sophisticated theories are valence bond theory which includes orbital hybridization and resonance, and the linear combination of atomic orbitals molecular orbital method which includes ligand field theory. Electrostatics are used to describe bond polarities and the effects they have on chemical substances.