Unit One: Atomic Theory/Configuration
... • PROTONS give an atom its identity. They are the ONLY subatomic particle that must be identical from one atom to another. Neutrons AND electrons can vary... • SO, how can we create ONE box on the periodic table to represent ALL atoms of an element? We must represent AVERAGE atoms. (That’s why the a ...
... • PROTONS give an atom its identity. They are the ONLY subatomic particle that must be identical from one atom to another. Neutrons AND electrons can vary... • SO, how can we create ONE box on the periodic table to represent ALL atoms of an element? We must represent AVERAGE atoms. (That’s why the a ...
Note - Science 10
... atom. Each shell holds a maximum number of electrons (2, 8, 8, 18, 18) Electrons in the outermost shell are called valence electrons If the valence shell is full = the atom is stable If the valence shell is not full = the atom is not stable Note: Think of the shells as being 3D like spheres, ...
... atom. Each shell holds a maximum number of electrons (2, 8, 8, 18, 18) Electrons in the outermost shell are called valence electrons If the valence shell is full = the atom is stable If the valence shell is not full = the atom is not stable Note: Think of the shells as being 3D like spheres, ...
Chapter 2: Atoms, Molecules, and Ions
... 3. Students will be able to state the number of protons, electrons and neutrons in neutral atoms, ions, and isotopes. 4. Students will understand the derivation and meaning of atomic mass and be able to calculate weighted average masses from isotopic data. 5. Students will become familiar with the w ...
... 3. Students will be able to state the number of protons, electrons and neutrons in neutral atoms, ions, and isotopes. 4. Students will understand the derivation and meaning of atomic mass and be able to calculate weighted average masses from isotopic data. 5. Students will become familiar with the w ...
Unit 13 - Electrochemistry
... Voltage: The potential difference or electromotive force, measured in volts; it represents the amount of work that moving an electric charge between two points would take. Electrode: A conductor used to establish electrical contact with a nonmetallic part of a circuit, such as an electrolyte. electr ...
... Voltage: The potential difference or electromotive force, measured in volts; it represents the amount of work that moving an electric charge between two points would take. Electrode: A conductor used to establish electrical contact with a nonmetallic part of a circuit, such as an electrolyte. electr ...
Chapter 4 Outline Onlevel 2013
... 1. Greeks - 400 B.C. a. Idea that matter could not be destroyed b. Believed that matter could be divided into smaller particles until a basic particle was reached c. Democritus called these particles “Atomos” for indivisible thus the name atoms 2. Atoms a. The smallest unit of an element that can ex ...
... 1. Greeks - 400 B.C. a. Idea that matter could not be destroyed b. Believed that matter could be divided into smaller particles until a basic particle was reached c. Democritus called these particles “Atomos” for indivisible thus the name atoms 2. Atoms a. The smallest unit of an element that can ex ...
Chapter 18 Comparing Atoms Lab
... In this investigation, you will investigate the structure of the atom and identify what makes atoms of different elements different from each other. We once believed that atoms were the smallest unit of matter. Then it was discovered that there are even smaller particles inside atoms (J.J. Thomson). ...
... In this investigation, you will investigate the structure of the atom and identify what makes atoms of different elements different from each other. We once believed that atoms were the smallest unit of matter. Then it was discovered that there are even smaller particles inside atoms (J.J. Thomson). ...
Balancing Chemical Equations
... original equations as a single atom. Think of this as a recipe and you can’t just start adding ingredients and expect the same result from the recipe. Ex. CH4 + O2 + O2 CO2 + H2O + H2O C=1 C=1 H=4 H=4 O=4 O=4 The correct way to write this is to put a coefficient to represent multiple molecules or ...
... original equations as a single atom. Think of this as a recipe and you can’t just start adding ingredients and expect the same result from the recipe. Ex. CH4 + O2 + O2 CO2 + H2O + H2O C=1 C=1 H=4 H=4 O=4 O=4 The correct way to write this is to put a coefficient to represent multiple molecules or ...
Density
... • Ionic Radius goes by the same rules as atomic radius (ions get larger as we move down and to the left). • However it is necessary to treat anions and cations separately. (Anions are ...
... • Ionic Radius goes by the same rules as atomic radius (ions get larger as we move down and to the left). • However it is necessary to treat anions and cations separately. (Anions are ...
Atoms
... had the best model of the atom so far, but Niels Bohr created a better and more useful model Bohr’s ...
... had the best model of the atom so far, but Niels Bohr created a better and more useful model Bohr’s ...
Chemistry I Exam
... to the distance covered. B. The speed of the bicycle remained constant throughout the entire duration of the trip. C. The distance travelled per hour is constant. D. The student rested for one hour half way through the trip. E. The graph is a curve rather than a straight line because the speed of th ...
... to the distance covered. B. The speed of the bicycle remained constant throughout the entire duration of the trip. C. The distance travelled per hour is constant. D. The student rested for one hour half way through the trip. E. The graph is a curve rather than a straight line because the speed of th ...
The Atom: Quick Note Guide
... Democritus Named the atom Dalton All matter is made up of small particles called atoms Atoms of a given element are identical in size and mass Atoms of different elements can physically/chemically combine to form compounds In reactions, atoms combine, separate, or rearrange Atoms cannot be divided, ...
... Democritus Named the atom Dalton All matter is made up of small particles called atoms Atoms of a given element are identical in size and mass Atoms of different elements can physically/chemically combine to form compounds In reactions, atoms combine, separate, or rearrange Atoms cannot be divided, ...
Cumulative Review, entire quarter
... For positive ions, remove electrons from the outer shell or period first. On the filling diagram , this would be row by row, from the top down. ...
... For positive ions, remove electrons from the outer shell or period first. On the filling diagram , this would be row by row, from the top down. ...
Chapter 4 Study Guide
... Chapter 4 Study Guide Know definitions for the following vocabulary words: matter spectral line atom energy level nucleus electron cloud proton electromagnetic spectrum neutron charge electron Thomson’s atomic model proportion Rutherford’s atomic model Democritus Bohr’s atomic model Dalton element L ...
... Chapter 4 Study Guide Know definitions for the following vocabulary words: matter spectral line atom energy level nucleus electron cloud proton electromagnetic spectrum neutron charge electron Thomson’s atomic model proportion Rutherford’s atomic model Democritus Bohr’s atomic model Dalton element L ...
final exam review chapter 1-4
... 5. If you have 4 g NaOH, and 10 g HBr, what is the limiting reagent and how much salt is produced? In lab if you produce1 g salt, what is the percent yield? ...
... 5. If you have 4 g NaOH, and 10 g HBr, what is the limiting reagent and how much salt is produced? In lab if you produce1 g salt, what is the percent yield? ...
Chemistry
... elements. (For example, at room temperature, chlorine is a gas and iodine is a solid.) Compare the strength of the forces of attraction between molecules of different elements. (For example, at room temperature, chlorine is a gas and iodine is a solid.) Compare the strength of the forces of attracti ...
... elements. (For example, at room temperature, chlorine is a gas and iodine is a solid.) Compare the strength of the forces of attraction between molecules of different elements. (For example, at room temperature, chlorine is a gas and iodine is a solid.) Compare the strength of the forces of attracti ...
Section 2: “The Structure of Atoms
... Section 2: “The Structure of Atoms” 4. On the periodic table, the atomic mass displayed is an average of the atomic masses of all of that element’s isotopes. 5. It is a weighted average so the mostly commonly found isotopes have the most impact on the mass. ...
... Section 2: “The Structure of Atoms” 4. On the periodic table, the atomic mass displayed is an average of the atomic masses of all of that element’s isotopes. 5. It is a weighted average so the mostly commonly found isotopes have the most impact on the mass. ...
ATOMS: THE BUILDING BLOCKS OF MATTER from the
... describe the motion of electrons. Quantum Theory - The theory that explains matter and energy at atomic and sub-atomic levels, sometimes called Quantum Mechanics. quarks - Sub-atomic particles of matter. There are six different types of quarks but only two occur in the nucleus of atoms. radioactive ...
... describe the motion of electrons. Quantum Theory - The theory that explains matter and energy at atomic and sub-atomic levels, sometimes called Quantum Mechanics. quarks - Sub-atomic particles of matter. There are six different types of quarks but only two occur in the nucleus of atoms. radioactive ...
Ionic and Covalent Bonding
... • Nonmetals tend to gain electrons or share electrons with another nonmetal to achieve a complete octet to form anions. ...
... • Nonmetals tend to gain electrons or share electrons with another nonmetal to achieve a complete octet to form anions. ...
Reactions
... • Chemical reaction – a process in which bonds of compounds are broken and reformed into different compounds • Molecules are rearranged during reactions, but composition stays the same • There are the same number of atoms in the products as there are in the reactants • Reactant – the starting materi ...
... • Chemical reaction – a process in which bonds of compounds are broken and reformed into different compounds • Molecules are rearranged during reactions, but composition stays the same • There are the same number of atoms in the products as there are in the reactants • Reactant – the starting materi ...
20150918145547
... • ______ predicted that the atoms of any element are different from the atoms of all other elements • Atomic Number – atoms of any given element always have the same number of protons – Atomic number of an _______ equals the number of protons in an atom of that element – _______ of different element ...
... • ______ predicted that the atoms of any element are different from the atoms of all other elements • Atomic Number – atoms of any given element always have the same number of protons – Atomic number of an _______ equals the number of protons in an atom of that element – _______ of different element ...
Etymology of Atom - New Academic Science
... Robert Andrews Milliken an American scientist greatly improved the method employed by Thomson for measuring directly the charge of an electron. In Milliken’s oildrop experiment (1909-1910), he produced microscopic droplets of an oil and observed them falling in the space between two electrically cha ...
... Robert Andrews Milliken an American scientist greatly improved the method employed by Thomson for measuring directly the charge of an electron. In Milliken’s oildrop experiment (1909-1910), he produced microscopic droplets of an oil and observed them falling in the space between two electrically cha ...
Resource for Final Exam Prep
... Intermolecular forces: London-dispersion (due to temporary dipole, this is the only force for non-polar molecules), dipole-dipole (polar molecules), ion-dipole (ions and polar molecule), hydrogen bonding (molecule should be H attached to F, O or N and there should be at least one lone pair of electr ...
... Intermolecular forces: London-dispersion (due to temporary dipole, this is the only force for non-polar molecules), dipole-dipole (polar molecules), ion-dipole (ions and polar molecule), hydrogen bonding (molecule should be H attached to F, O or N and there should be at least one lone pair of electr ...
Chapter 1 Review Sheet
... 1. element – the most simple form of matter that can’t be broken down by either chemical or physical means 2. compound – two or more elements that are chemically combined 3. atom – the smallest representative part of an element 4. atomic mass unit – the unit used to measure the relative mass of atom ...
... 1. element – the most simple form of matter that can’t be broken down by either chemical or physical means 2. compound – two or more elements that are chemically combined 3. atom – the smallest representative part of an element 4. atomic mass unit – the unit used to measure the relative mass of atom ...
History of molecular theory
In chemistry, the history of molecular theory traces the origins of the concept or idea of the existence of strong chemical bonds between two or more atoms.The modern concept of molecules can be traced back towards pre-scientific Greek philosophers such as Leucippus who argued that all the universe is composed of atoms and voids. Circa 450 BC Empedocles imagined fundamental elements (fire (20px), earth (20px), air (20px), and water (20px)) and ""forces"" of attraction and repulsion allowing the elements to interact. Prior to this, Heraclitus had claimed that fire or change was fundamental to our existence, created through the combination of opposite properties. In the Timaeus, Plato, following Pythagoras, considered mathematical entities such as number, point, line and triangle as the fundamental building blocks or elements of this ephemeral world, and considered the four elements of fire, air, water and earth as states of substances through which the true mathematical principles or elements would pass. A fifth element, the incorruptible quintessence aether, was considered to be the fundamental building block of the heavenly bodies. The viewpoint of Leucippus and Empedocles, along with the aether, was accepted by Aristotle and passed to medieval and renaissance Europe. A modern conceptualization of molecules began to develop in the 19th century along with experimental evidence for pure chemical elements and how individual atoms of different chemical substances such as hydrogen and oxygen can combine to form chemically stable molecules such as water molecules.