Counting atoms1
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The document provides instructions and information for several chemistry-related tasks, including picking up materials from the materials manager, returning items after a time limit, and filling in a chart. It also explains the formula for compounds, indicating the elements and number of atoms present, and provides examples of compound formulas like calcium carbonate, magnesium hydroxide, and trinitrotoluene. The main elements that make up living organisms are identified as carbon, hydrogen, oxygen, nitrogen, phosphorus, and sulfur.
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Counting Atoms Day 1
The document provides information about compounds and their formulas. It explains that subscripts in formulas indicate the number of atoms present of each element in a compound. Examples are given of common compounds like calcium carbonate (CaCO3), magnesium hydroxide (Mg(OH)2), and trinitrotoluene explosive (C7H5(NO2)3). The main elements that make up living organisms are identified as carbon, phosphorus, hydrogen, oxygen, nitrogen and sulfur. The document also lists common unit labels for mass, volume, and density.
Counting Atoms Day 2
This document provides instructions and materials for a class, including:
1) Requiring students to bring specific worksheets and cards to class on Friday.
2) Reminding students they have new seats.
3) Covering that the main elements in living organisms are carbon, hydrogen, oxygen, nitrogen, phosphorus, and sulfur.
Counting Atoms
This document provides instructions for an assignment on counting atoms. It lists the materials needed, which include a pen or pencil, colored pencils/markers/highlighters, and an atoms counting booklet. It explains that quick writes will not be graded but used for participation and honesty. Students can use their brain, class notes, labs, or worksheets, but not the textbook or interactive reader. They have 10 minutes to complete as many questions as possible using a periodic table. Students will self-grade with a colored pencil. The document then provides examples of chemical formulas and their breakdown of elements and subscripts. It notes the main elements in living organisms are carbon, hydrogen, nitrogen, oxygen, phosphorus, and sulfur
Counting Atoms - Day 1
The document provides instructions and information about an upcoming science lesson on atoms and elements. It includes:
- Instructions for an oral presentation on a student-chosen element where they will describe its atom model, number of protons/neutrons/electrons, element type, and state at room temperature.
- Information about counting atoms in chemical formulas, including examples of calcium carbonate, magnesium hydroxide, and trinitrotoluene.
- A chart for students to complete with the mass and volume unit labels.
- Instructions that any outstanding homework is due by the end of the next period.
Counting Atoms Day
The document discusses atoms and counting atoms in compounds. It provides examples of chemical formulas and how to determine the number of each type of atom present. Students are asked to complete an oral presentation on an element describing its atom model, number of protons, neutrons and electrons, and state at room temperature. The main elements that make up living organisms are identified as carbon, hydrogen, nitrogen, oxygen, phosphorus and sulfur.
Balance
This document contains a chemistry assignment with multiple parts. It begins with 15 chemical equations to balance. Then it provides an equation for lithium nitride reacting with water and asks 5 questions about mole ratios and amounts needed to produce certain amounts of products. Next is another equation to balance and 6 additional questions about amounts needed to produce an amount of one product. Finally, there are answers provided to balance the initial 15 equations and to the other questions asked.
Definition of Matter Lab Day 2
This document provides an overview of today's science class which includes:
1) Materials needed like pencils, log books, and textbooks.
2) Reminders about test corrections, power notes, and retakes.
3) A series of review questions about the key characteristics and changes between the different states of matter.
4) An activity where students will sort matter and play a levels game to learn about physical properties.
5) An activity where students will shade their periodic table to identify liquids, gases and solids.
6) A math lesson on finding percents from fractions.
7) The homework assigned which is test corrections and scheduling retakes if needed.
Balancing equations
The document provides a 7-step process for balancing chemical equations: 1) check for diatomic molecules, 2) balance metals, 3) balance nonmetals, 4) balance oxygen, 5) balance hydrogen, 6) recount all atoms, 7) reduce coefficients to lowest whole numbers. It then lists example chemical equations to balance using the 7 steps and provides practice problems for balancing additional equations.
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Counting Atoms Day 1
The document provides information about compounds and their formulas. It explains that subscripts in formulas indicate the number of atoms present of each element in a compound. Examples are given of common compounds like calcium carbonate (CaCO3), magnesium hydroxide (Mg(OH)2), and trinitrotoluene explosive (C7H5(NO2)3). The main elements that make up living organisms are identified as carbon, phosphorus, hydrogen, oxygen, nitrogen and sulfur. The document also lists common unit labels for mass, volume, and density.
Counting Atoms Day 2
This document provides instructions and materials for a class, including:
1) Requiring students to bring specific worksheets and cards to class on Friday.
2) Reminding students they have new seats.
3) Covering that the main elements in living organisms are carbon, hydrogen, oxygen, nitrogen, phosphorus, and sulfur.
Counting Atoms
This document provides instructions for an assignment on counting atoms. It lists the materials needed, which include a pen or pencil, colored pencils/markers/highlighters, and an atoms counting booklet. It explains that quick writes will not be graded but used for participation and honesty. Students can use their brain, class notes, labs, or worksheets, but not the textbook or interactive reader. They have 10 minutes to complete as many questions as possible using a periodic table. Students will self-grade with a colored pencil. The document then provides examples of chemical formulas and their breakdown of elements and subscripts. It notes the main elements in living organisms are carbon, hydrogen, nitrogen, oxygen, phosphorus, and sulfur
Counting Atoms - Day 1
The document provides instructions and information about an upcoming science lesson on atoms and elements. It includes:
- Instructions for an oral presentation on a student-chosen element where they will describe its atom model, number of protons/neutrons/electrons, element type, and state at room temperature.
- Information about counting atoms in chemical formulas, including examples of calcium carbonate, magnesium hydroxide, and trinitrotoluene.
- A chart for students to complete with the mass and volume unit labels.
- Instructions that any outstanding homework is due by the end of the next period.
Counting Atoms Day
The document discusses atoms and counting atoms in compounds. It provides examples of chemical formulas and how to determine the number of each type of atom present. Students are asked to complete an oral presentation on an element describing its atom model, number of protons, neutrons and electrons, and state at room temperature. The main elements that make up living organisms are identified as carbon, hydrogen, nitrogen, oxygen, phosphorus and sulfur.
Balance
This document contains a chemistry assignment with multiple parts. It begins with 15 chemical equations to balance. Then it provides an equation for lithium nitride reacting with water and asks 5 questions about mole ratios and amounts needed to produce certain amounts of products. Next is another equation to balance and 6 additional questions about amounts needed to produce an amount of one product. Finally, there are answers provided to balance the initial 15 equations and to the other questions asked.
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This document provides an overview of today's science class which includes:
1) Materials needed like pencils, log books, and textbooks.
2) Reminders about test corrections, power notes, and retakes.
3) A series of review questions about the key characteristics and changes between the different states of matter.
4) An activity where students will sort matter and play a levels game to learn about physical properties.
5) An activity where students will shade their periodic table to identify liquids, gases and solids.
6) A math lesson on finding percents from fractions.
7) The homework assigned which is test corrections and scheduling retakes if needed.
Balancing equations
The document provides a 7-step process for balancing chemical equations: 1) check for diatomic molecules, 2) balance metals, 3) balance nonmetals, 4) balance oxygen, 5) balance hydrogen, 6) recount all atoms, 7) reduce coefficients to lowest whole numbers. It then lists example chemical equations to balance using the 7 steps and provides practice problems for balancing additional equations.
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1. Students are to complete pages from a "Counting Atoms + Density Review" worksheet and turn it in at the start of class tomorrow.
2. Flashcards numbered 31-60 from the "STAR CARDS" set are due at the start of class on Friday.
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Organic molecules contain carbon skeletons. Alkanes contain only carbon and hydrogen atoms. Pentane has the molecular formula C5H12. Alkanes react with oxygen to produce carbon dioxide and water. Alcohols contain the hydroxyl group and ethanol has the molecular formula C2H5OH. Alcohols are used as solvents and antiseptics. Alcohols react with sodium and oxygen. Larger alcohols do not mix with water due to intermolecular forces. Carboxylic acids contain the carboxyl group and sweaty smells are caused by butanoic acid. Carboxylic acids react with sodium, potassium hydroxide, and sodium carbonate.
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Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions. It is based on the law of conservation of mass, which states that mass is conserved in chemical reactions. The balanced chemical equation for the reaction of iron and oxygen shows that four moles of iron react with three moles of oxygen to produce two moles of iron(III) oxide. While the chemical equation does not show masses, the mole quantities can be converted to masses by using molar masses. The total mass of reactants must equal the total mass of products, according to the law of conservation of mass.
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This activity is designed to introduce a convenient unit used by.docx
This activity is designed to introduce a convenient unit used by chemists and to illustrate uses of the unit.
Part I: What Is a Mole And Why Are Chemists Interested in It?
Counting things is a normal part of everyday life. How many days left until vacation? How many eggs do I need for the recipe? If large numbers of things are involved, we use grouping
strategies to make the numbers easier to manage. For example, 4 more
weeks
until vacation, tells
us that there are twenty-eight days. One
dozen
eggs is the common way of expressing the quantity
12.
Half of a dozen of anything would be 6 units. One
gross
is 144 items (12 dozen) and a
ream
of paper contain 500 sheets.
Chemist are faced with a unique problem when dealing with numbers of atoms or molecules. The particles are so small that any amount of them that we are able to physically handle contains a number of particles so large that there is nothing else in our experience that contains so many units. This
incredibly
large number calls for a special counting group -
the MOLE.
A
MOLE
is
6.022
x
1023
particles
. This is often referred to as
Avogadro=s
number
. Let=s make sure we understand how big this is. One mole of the element carbon has a mass of 12.01 grams. The smallest particle of an element is an atom. So one mole of carbon contains 602,200,000,000,000,000,000,000 atoms of carbon.
Look for the element carbon on the periodic table. Do you notice anything special about the value 12.01? Explain
The mass of one mole of the element magnesium is 24.30 grams. How many atoms does a sample of magnesium with a mass of 24.30 grams contain?
Stated in general terms, the mass of one mole of any element is equal to the
of that element expressed in grams. The mass of a mole of any element can be found by looking on .
The mass of 0.5000 moles of carbon is and contains
atoms of carbon.
Remember when dividing numbers written in scientific notation the number portion is divided
normally and the exponents are subtracted.
6.022x1023
divided by 2 is the same as 6.022 x1023/2
x
100.
So the answer is found by dividing 6.022 by 2 = 3.011 and the subtracting exponent 0
from exponent 23.
The answer in scientific notation is 3.011x1023
atoms
of carbon.
Calculator tip
: for exponential notation use the EE or EXP key (not 10^)
If you have a bottle containing 8.10 grams of magnesium, how many Mg atoms are present in the bottle? Show your work. What is different about this problem compared to the last one involving carbon?
Remember that some elements, when alone, exist in the form of diatomic molecules: H2, O2, N2, I2, F2, Cl2, Br2, Their smallest piece is a molecule containing two atoms. If one mole of oxygen were required for an experiment you would be using O2 the gas. One mole of O2 would have a mass of
and contain particles (molecules).
The characteristic unit of the compound CO2 is a molecule. Each CO2 molecule has atoms. In order to find the mass .
Chemistry - Chp 12 - Stoichiometry - Notes
When 20.0 g of FeS2 reacts with 16.0 g of O2 according to the balanced equation 4FeS2 + 15O2 → 2Fe2O3 + 8SO3:
- O2 is the limiting reagent because it produces the least amount of SO3.
- Using stoichiometry calculations, 16.0 g of O2 can produce 8.0 g of SO3.
- Therefore, the amount of SO3 produced is 8.0 g.
The periodic table presentation for 4050 [autosaved]
The document provides information about the periodic table including:
- The periodic table organizes elements according to their atomic number and valence electrons.
- Elements in the same column have similar chemical properties.
- The periodic table has been developed and improved over time by scientists like Dmitri Mendeleev and Lothar Meyer to better organize the known elements.
- The periodic table is an essential tool for chemists as it provides key information about elements like their atomic number, mass, configuration, and reactivity.
C2f Clean Air
The atmosphere is mainly composed of nitrogen, oxygen, and carbon dioxide. The carbon cycle involves photosynthesis, respiration, and combustion and works to maintain stable levels of oxygen and carbon dioxide. Early in Earth's formation, volcanoes released gases like carbon dioxide, water vapor, and ammonia into the atmosphere. Over time, the formation of oceans and evolution of plants increased oxygen levels while decreasing carbon dioxide. Human activities like increased population, fossil fuel combustion, deforestation, and transportation have led to higher atmospheric pollution levels and their associated health and environmental impacts. Strategies to control pollution include emissions standards, catalytic converters, and reducing carbon dioxide emissions.
the mathematics of chemistry stoichiometry dimensional analysis.ppt
Here is a stoichiometry question I wrote for the given reaction:
If 3.25 grams of barium chloride are available to react, how many grams of barium sulfate can be produced?
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This document provides instructions and materials for a science class. Students are asked to:
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2) Work in groups and individually reflect on what went well and could be improved in their cooperative learning experience.
3) Draw Bohr models of various elements using information from the periodic table, including lithium, magnesium, and oxygen.
4) Review the first page of their notes and complete homework which includes minimum days the next two days and having their binder checked the following Wednesday.
Intro to atoms (edited for 2018)
Here are the answers to the cold call questions:
1. The three subatomic particles in an atom are protons (with a positive charge of +1), neutrons (with no charge), and electrons (with a negative charge of -1).
2. The two subatomic particles found in the nucleus of an atom are protons and neutrons.
3. Electrons are found orbiting the nucleus of an atom.
4. The number of protons determines the chemical element of an atom.
5. A valence electron is an electron in the outermost electron shell of an atom that is involved in bonding with other atoms.
6. Atomic mass is the average mass of all the known isotopes of
Stoichiometry PowerPoint
This document provides an overview of moles, molar mass, and stoichiometry. It defines a mole as 6.02x1023 particles of an element or compound. Avogadro's number is equal to this quantity of particles. Molecular mass is the mass of one molecule in atomic mass units (amu) while molar mass is the mass of one mole of a substance in grams. Examples are given for calculating molecular and molar mass. The document then discusses balancing chemical equations and using molar ratios from balanced equations to solve stoichiometry problems involving moles, grams, and particles of reactants and products.
Chemistrychapter3 111004105015-phpapp02
The document discusses atomic structure and the building blocks of matter. It defines key terms like atoms, subatomic particles, isotopes, and moles. It explains that atoms of the same element are distinguished by their number of protons. The mole is introduced as a unit used to measure amount of substance equal to 6.02x1023 particles. Examples are given for calculating molar mass and empirical formulas from elemental composition data.
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Here are the conversions with work shown:
1) 45.5 inches ÷ 12 inches/foot = 3.79 feet
2) 0.550 gal × 4 qt/gal × 2 pints/qt × 16 oz/pint = 896 oz
3) 14,259 feet ÷ 5,280 feet/mile = 2.70 miles
Chemistry - Chp 20 - Oxidation Reduction - Notes
Oxidation and reduction reactions, also called redox reactions, involve the transfer of electrons between reactants. In redox reactions, one reactant gets oxidized by losing electrons while another reactant gets reduced by gaining electrons. The reactant that loses electrons is the oxidizing agent, while the reactant that gains electrons is the reducing agent. Redox reactions can be identified by changes in oxidation numbers, which are assigned to track electron gains and losses. Balancing redox equations requires splitting the overall reaction into separate half-reactions for oxidation and reduction, then combining the half-reactions by adding electrons to balance charges.
Fractional Distillation Lesson Resource
Fractional distillation is the process of separating crude oil into its different hydrocarbon fractions based on differences in boiling points. Crude oil is heated in a fractional distillation column, where the lighter hydrocarbon chains evaporate first and condense at the top, while heavier chains remain lower down. This allows fractions like gasoline and kerosene to be isolated for use as fuels or feedstocks. Balancing chemical equations is important for showing the conservation of mass during combustion reactions that produce energy, carbon dioxide, and water from hydrocarbon fuels and oxygen.
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This document provides instructions and information for a lesson on density including:
1) Materials needed such as pencils and a density chart
2) Directions to copy the density chart into notes and calculate the density of samples
3) Assigning group roles for an oral presentation such as managers and materials managers
Similar to Counting atoms1 (20)
This activity is designed to introduce a convenient unit used by.docx
This activity is designed to introduce a convenient unit used by.docx
The periodic table presentation for 4050 [autosaved]
The periodic table presentation for 4050 [autosaved]
the mathematics of chemistry stoichiometry dimensional analysis.ppt
the mathematics of chemistry stoichiometry dimensional analysis.ppt
Balancing Chemical Equations Powerpoint General Chemistry 1
Balancing Chemical Equations Powerpoint General Chemistry 1
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Counting atoms1
- 1. You Will Need: 1. Bohr Model Drawings & Density Review – Due Now 2. Atoms-Building Blocks of Matter – Counting Atoms Bookshelf – Please Staple
- 2. You Will Need: 1. One Pencil 2. Materials Manager – Pick up One Periodic Table 3. Oral Presenters – What is your team’s Table Number & Wager? 4. Managers – Fill in Chart 5. Timer Designers – Return Final Jeopardy and P.T. after 2 minutes
- 3. The formula for a compound indicates the elements that make up the compound and the number of atoms of each element present in that specific compound. These numbers of atoms are indicated by the use of small numbers called subscripts.
- 4. When a subscript appears outside the parentheses, it indicates that all the elements inside the parentheses should be multiplied by that subscript. Fe(OH) 3
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- 6. • Magnesium Hydroxide Mg(OH)2 Mg = Magnesium= 1 O = Oxygen= 2 H = Hydrogen= 2
- 7. Trinitrotoluene = (TNT) explosive C7H5(NO2)3 C= Carbon = 7 H = Hydrogen = 5 N = Nitrogen = 3 O = Oxygen = 6
- 8. As you look over these compounds you may observe that many of them contain atoms similar _________ of elements. Since carbon we are a ______________ based environment, carbon is found in all living organisms. The elements in the Human Body can be broken down to include the main elements of Hydrogen, Oxygen, Nitrogen, Carbon and representatives from about 20 other elements.
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- 10. grams •Mass Unit Label =_______________ cm 3 •Volume Unit Labels = ________, mL cc _______ or _______as a unit label g/cm 3 •Density unit label = ___________, g/mL g/cc ________ or __________
- 11. 5 points given: • 2 points for the problem you are inputting into the calculator • 2 points for the answer rounded to the nearest hundreth • 1 point for the unit label
- 12. 1. Counting Atoms – Due Tuesday-April 2nd 2. Enjoy your SPRING BREAK!