General Chemistry
... It is possible for more than one pair of electrons to be shared between two atoms (multiple bonds): Single covalent bond: One shared pair of electrons = single bond (e.g. H2); H-H Double covalent bond: Two shared pairs of electrons = double bond (e.g. O2); O=O Triple covalent bond: Three shared pair ...
... It is possible for more than one pair of electrons to be shared between two atoms (multiple bonds): Single covalent bond: One shared pair of electrons = single bond (e.g. H2); H-H Double covalent bond: Two shared pairs of electrons = double bond (e.g. O2); O=O Triple covalent bond: Three shared pair ...
8th Grade: First Semester Final Review
... Choose the letter of the term that matches it correctly. Each term is used only once. a. halogen d. oxygen and nitrogen b. noble gases e. carbon c. metalloids 29. do not form natural compounds 32. nonmetals in your body 30. nonmetal from group 14 33. semiconductors 31. reacts with a metal to form a ...
... Choose the letter of the term that matches it correctly. Each term is used only once. a. halogen d. oxygen and nitrogen b. noble gases e. carbon c. metalloids 29. do not form natural compounds 32. nonmetals in your body 30. nonmetal from group 14 33. semiconductors 31. reacts with a metal to form a ...
Things to Know to Pass the Chemistry Regents
... 15. Rutherford’s gold foil showed atoms small (+) nucleus & mostly empty space with e*few deflections = small (+) nucleus, most through = mostly empty space 16. Bohr’s model e- in orbits like planets around sun (orbit does NOT equal orbital) 17. Modern, wave-mechanical model e- in orbitals (most pro ...
... 15. Rutherford’s gold foil showed atoms small (+) nucleus & mostly empty space with e*few deflections = small (+) nucleus, most through = mostly empty space 16. Bohr’s model e- in orbits like planets around sun (orbit does NOT equal orbital) 17. Modern, wave-mechanical model e- in orbitals (most pro ...
sch3u unit 1 test: matter
... 1. Beakers A and B are filled with substances that are liquid at room temperature. The substance in beaker A experiences London dispersion forces. The substance in beaker B experience dipole-dipole interactions. Compare and contrast the two force types. Which substance will boil at a lower temperatu ...
... 1. Beakers A and B are filled with substances that are liquid at room temperature. The substance in beaker A experiences London dispersion forces. The substance in beaker B experience dipole-dipole interactions. Compare and contrast the two force types. Which substance will boil at a lower temperatu ...
Document
... 21. The __________ _____________ tells you how many electrons an atom must gain, lose, or share to become stable. 22. Numbers that precede symbols and formulas in a chemical equation are ______________. 23. A chemical reaction in which two or more substances combine to form another substance is call ...
... 21. The __________ _____________ tells you how many electrons an atom must gain, lose, or share to become stable. 22. Numbers that precede symbols and formulas in a chemical equation are ______________. 23. A chemical reaction in which two or more substances combine to form another substance is call ...
Ground State
... Pieter Zeeman, Lorentz “spectra line splitting” in magnetic filed 1902 Nobel Prize ...
... Pieter Zeeman, Lorentz “spectra line splitting” in magnetic filed 1902 Nobel Prize ...
Chapter 7 Handout 1 Atomic Orbitals Quantum Numbers: Principal
... Rules for filling orbitals: 1. Aufbau Principle: a. Electrons fill up orbitals of lowest energy first b. Orbitals in the same sublevel are equal in energy c. Sometimes energy levels overlap 2. Pauli Exculsion Principle a. There is a max of 2 electrons in any one orbital b. These 2 electrons must ha ...
... Rules for filling orbitals: 1. Aufbau Principle: a. Electrons fill up orbitals of lowest energy first b. Orbitals in the same sublevel are equal in energy c. Sometimes energy levels overlap 2. Pauli Exculsion Principle a. There is a max of 2 electrons in any one orbital b. These 2 electrons must ha ...
Unit 1 – Physical Science and Chemical Reactions
... ion: a charged atom Formed when a metal loses electrons to form a positive ion (cation) or when non-metals gain electrons to form a negative ion (anion) All atoms gain/lose electrons to become like the nearest noble gas (become stable) When naming ions: Metal (cation) names: stay the same No ...
... ion: a charged atom Formed when a metal loses electrons to form a positive ion (cation) or when non-metals gain electrons to form a negative ion (anion) All atoms gain/lose electrons to become like the nearest noble gas (become stable) When naming ions: Metal (cation) names: stay the same No ...
Chemistry 215 Quiz 1 (20 points)
... Given the equation S (s) + O2 (g) SO2 (g), H = -296 kJ, which of the following statements is FALSE? a) The reaction is exothermic. b) When 1 mole sulfur is reacted, 296 kJ of energy is released. c) This is a combustion reaction d) The standard enthalpy of formation for SO2 (g) is –296 kJ e) Heat ...
... Given the equation S (s) + O2 (g) SO2 (g), H = -296 kJ, which of the following statements is FALSE? a) The reaction is exothermic. b) When 1 mole sulfur is reacted, 296 kJ of energy is released. c) This is a combustion reaction d) The standard enthalpy of formation for SO2 (g) is –296 kJ e) Heat ...
List Definition Chemistry - A Level / Secondary Chemistry Tuition
... van der Waals’ forces (induced dipole-induced dipole bonding) exist when non-polar R groups (e.g. alkyl or aryl groups) come close together. They are usually found on the inside of globular proteins where, because they are hydrophobic, they do not interfere with solubility. hydrogen bonding betw ...
... van der Waals’ forces (induced dipole-induced dipole bonding) exist when non-polar R groups (e.g. alkyl or aryl groups) come close together. They are usually found on the inside of globular proteins where, because they are hydrophobic, they do not interfere with solubility. hydrogen bonding betw ...
Mr. Knittel`s Final Review Sheet I Answers
... in which negative charges were stuck into a positive blob, like plums in plum pudding. Although Thomson didn’t find evidence of the positive charges, he reasoned they must be there to balance the negatives. When Rutherford discovered the nucleus, Thomson’s model had to be refined further. Rutherford ...
... in which negative charges were stuck into a positive blob, like plums in plum pudding. Although Thomson didn’t find evidence of the positive charges, he reasoned they must be there to balance the negatives. When Rutherford discovered the nucleus, Thomson’s model had to be refined further. Rutherford ...
Practice Bypass Answers
... H2O – water is a polar covalent compound because two lone pairs on the oxygen and two bonding pairs between oxygen and hydrogen atoms repel each other causing water molecule to obtain bent shape; also, oxygen has significantly higher electronegativity (attraction for shared electrons) than hydrogen ...
... H2O – water is a polar covalent compound because two lone pairs on the oxygen and two bonding pairs between oxygen and hydrogen atoms repel each other causing water molecule to obtain bent shape; also, oxygen has significantly higher electronegativity (attraction for shared electrons) than hydrogen ...
Chp 1,2 rev
... Give the names of the shapes of molecules below HI BF3 CI4 NH3 H2O SO2 What is hybridization? How many sets of electrons are around the central atom if its sp3 hybridized? Sp2? ...
... Give the names of the shapes of molecules below HI BF3 CI4 NH3 H2O SO2 What is hybridization? How many sets of electrons are around the central atom if its sp3 hybridized? Sp2? ...
Chemistry Review - pams-hoey
... Atomic Number and Mass • The number of protons in the nucleus determines the atomic number of the element • The mass number is the sum of the protons and neutrons and is used to distinguish one isotope from another • Atomic mass is the average mass of all the isotopes of an element ...
... Atomic Number and Mass • The number of protons in the nucleus determines the atomic number of the element • The mass number is the sum of the protons and neutrons and is used to distinguish one isotope from another • Atomic mass is the average mass of all the isotopes of an element ...
Term paper
... In first case, the electron probability is mostly between the nucleii while in second case, it is outside. So, (+) is more stable. We can extend our calculations to p-orbitals and we find similar wave functions. But, other orbitals have directional character. When, pz has formed σ bond, there is lat ...
... In first case, the electron probability is mostly between the nucleii while in second case, it is outside. So, (+) is more stable. We can extend our calculations to p-orbitals and we find similar wave functions. But, other orbitals have directional character. When, pz has formed σ bond, there is lat ...
Exam Review – Part 1
... Forming Stable Ions • To become stable some atoms will gain or lose electrons to form an ion • For an atom to become stable, it must look like a noble gas • That is, they must have a full outer (valence) shell of electrons (stable octet) ...
... Forming Stable Ions • To become stable some atoms will gain or lose electrons to form an ion • For an atom to become stable, it must look like a noble gas • That is, they must have a full outer (valence) shell of electrons (stable octet) ...
CHM134 General Chemistry I Semester Review – Dr. Steel This list
... 21. If n = 3, what are the allowed quantum numbers for l? 22. What element has the ground state electron configuration: [Ar]4s13d5? 23. What element has the ground state electron configuration: [Kr]5s2? 24. What is the maximum number of electrons permitted in a d sublevel? 25. Green light has a wave ...
... 21. If n = 3, what are the allowed quantum numbers for l? 22. What element has the ground state electron configuration: [Ar]4s13d5? 23. What element has the ground state electron configuration: [Kr]5s2? 24. What is the maximum number of electrons permitted in a d sublevel? 25. Green light has a wave ...
Test #5 Review
... Which force holds the nucleus together? the strong force Which force holds the electrons around the nucleus? the electromagnetic force Define mass number. number of protons + number of neutrons ...
... Which force holds the nucleus together? the strong force Which force holds the electrons around the nucleus? the electromagnetic force Define mass number. number of protons + number of neutrons ...
Lectures p block elements 3 hypervalency
... The concept of hypervalency in p block compounds A hypervalent molecule may be defined as a molecule in which there are more than four pairs of electrons around the central atom in the conventional Lewis diagram of the molecule. J. I Musher in 1969 originally defined hypervalent molecules as those ...
... The concept of hypervalency in p block compounds A hypervalent molecule may be defined as a molecule in which there are more than four pairs of electrons around the central atom in the conventional Lewis diagram of the molecule. J. I Musher in 1969 originally defined hypervalent molecules as those ...
Chapter-2-Human-Chemistry
... and bases reacting with one another • Dissociates itself into cations and anions when dissolved in water • Important for tissue strength, blood, and lymph ...
... and bases reacting with one another • Dissociates itself into cations and anions when dissolved in water • Important for tissue strength, blood, and lymph ...
Fall Semester Review Packet
... 9. Describe how the current periodic table is arranged by comparing groups, periods and properties of the elements. 10. Explain the difference between a molecule (covalent compound) and an ionic compound. Include the interaction between valence electrons and the types of bonds for each. 11. There ar ...
... 9. Describe how the current periodic table is arranged by comparing groups, periods and properties of the elements. 10. Explain the difference between a molecule (covalent compound) and an ionic compound. Include the interaction between valence electrons and the types of bonds for each. 11. There ar ...
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.