The Atom for Middle School - Miss Littles Classroom Website
atom: the smallest particle of an element that has all the properties of that element The atom has nocharge The 3 main subatomic particles that make up the atom are the proton, neutron and electron nucleus: small, dense positively charged center of an atom protons and neutrons are found in the nucleus
Atoms, Molecules and Matter: The Stuff of Chemistry
Nov 10, 2011 · 2 1 The ideal gas: a simple model 2 2 Temperature and thermometers 2 3 The equation of state Chapter 3 Chemical Reactions 3 1 Work, Heat, and Energy 3 2 Energy changes in reactions Chapter 4 A deeper look at the ideal gas 4 1 Back to basics: the laws of large numbers 4 2 Probability densities 4 3 Maxwell’s distribution law
SCIENCE (52) - CISCE
Definition of an atom • Constituents of an atom nucleus - (protons, neutrons) with associated electrons; mass number, atomic number • Electron distribution in the orbits - 2n 2 rule, Octet rule Reason for chemical activity of an atom • Definition and examples of isotopes (hydrogen, carbon, chlorine) (ii) Electrovalent and covalent
SCIENCE (52) CHEMISTRY SCIENCE Paper - 2
(i) Structure of an Atom, mass number and atomic number, Isotopes and Octet Rule • Definition of an atom • Constituents of an atom nucleus - (protons, neutrons) with associated electrons; mass number, atomic number • 2 Electron distribution in the orbits - 2n rule, Octet rule Reason for chemical activity of an atom Definition and
Atomic Packing Factor for Simple Cubic
Atomic Packing Factor for Simple Cubic :- no of atoms = 1 π volume of one atom = volume of unit cell (cubic) = a3 when , )a = 2r (Filling Factor = ( ) Atomic Filling Factor for BCC:-no of atoms =2 π volume of tow atoms =2*
Chapter Outline Diffusion - how do atoms move through solids
Interstitial atom before jump Interstitial atom after jump Interstitial diffusion is generally faster than vacancy diffusion because bonding of interstitials to the surrounding atoms is normally weaker and there are many more interstitial sites than vacancy sites to jump to Requires small impurity atoms (e g C, H, O) to fit into interstices
Example Exercise 91 Atomic Mass and Avogadro’s Number
(a) 1 atom of Au (b) 6 02 × 1023 atoms of Au Answers: (a) 196 97 amu; (b) 196 97 g Practice Exercise What is the mass of an average platinum atom? What is the mass of Avogadro’s number of Pt atoms? Answer: See Appendix G Concept Exercise
Experiment 7: Spectrum of the Hydrogen Atom
spectrum of the hydrogen atom It was the birth of Quantum Mechanics He hypothesizes that the angular momentum of an electron in orbit around a proton is quantized (i e it can only be a discrete multiple of a certain number): Under this simple assumption he managed to compute the energy of the electron around the atom:
C arbohydrates: Simple Sugars and Complex Chains
oxygen atom for every one carbon atom (CH 2 O) Two or more sugar mol-ecules can be assembled to form increasingly complex carbohydrates The two main types of carbohydrates in food are simple carbohydrates (sugars) and complex carbohydrates (starches and fi ber) SimpeS l ugars
[PDF] atome de fluor
[PDF] constitution de l'atome
[PDF] les isotopes definition
[PDF] isotope oxygène
[PDF] isotope exemple
[PDF] isotopes de l'hélium
[PDF] isotopes du carbone
[PDF] ordre de grandeur tissu
[PDF] chlore configuration électronique
[PDF] représentation de lewis du fer
[PDF] structure electronique fer 2+
[PDF] structure electronique du fer
[PDF] taille globule blanc
[PDF] taille d'un cheveux
© 2011 Pearson Education, Inc.Introductory Chemistry: Concepts and Critical Thinking, 6th Edition
Charles H. Corwin
Example Exercise 9.1Atomic Mass and Avogadro's NumberThe atomic mass of each element is listed below the symbol of the element in the periodic table: Cu =
63.55 amu, Hg = 200.59 amu, S = 32.07 amu, and He = 4.00 amu. The mass of Avogadro's number of atoms
is the atomic mass expressed in grams. Therefore, 6.02 10 23atoms of (a)Cu = 63.55 g(c)S = 32.07 g (b)Hg = 200.59 g(d)He = 4.00 g
Solution
Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro's
number of atoms for each of the following elements: (a)Copper(c)sulfur (b)Mercury(d)helium Refer to the periodic table and state the mass for each of the following: (a)1 atom of Au(b)6.02 1023 atoms of Au
Answers:(a) 196.97 amu; (b) 196.97 g
Practice Exercise
What is the mass of an average platinum atom? What is the mass of Avogadro's number of Pt atoms?Answer:See Appendix G.
Concept Exercise
© 2011 Pearson Education, Inc.Introductory Chemistry: Concepts and Critical Thinking, 6th EditionCharles H. Corwin
Example Exercise 9.2Mole Calculations I
Calculate the number of sodium atoms in 0.120 mol Na.Strategy Plan
Step 1: What unit is asked for in the answer?
Step 2: What given value is related to the answer?Step 3: What unit factor(s) should we apply?
Since 1 mol Na = 6.02
10 23atoms Na, the two unit factors are 1 mol Na/6.02 1023 atoms Na, and its reciprocal 6.02 10 23
atoms Na/1 mol Na.
Unit Analysis Map
© 2011 Pearson Education, Inc.Introductory Chemistry: Concepts and Critical Thinking, 6th EditionCharles H. Corwin
Example Exercise 9.2Mole Calculations I
Calculate the number of formula units in 0.0763 mol of sodium chloride, NaCl.Answers:4.59
10 22formula units NaCl
Practice Exercise
What is the number of molecules in 1.00 mol of any gas?Answer:See Appendix G.
Concept Exercise
We apply the unit factor 6.02 10
23atoms Na/1 mol Na to cancel moles , which appears in the denominator.
The answer is rounded to three digits because the given value and unit factor each have three significant
digits.Solution
Continued
© 2011 Pearson Education, Inc.Introductory Chemistry: Concepts and Critical Thinking, 6th EditionCharles H. Corwin
Example Exercise 9.3Mole Calculations I
Calculate the number of moles of potassium in 1.2510 21atoms K.
Strategy Plan
Step 1: What unit is asked for in the answer?
Step 2: What given value is related to the answer?Step 3: What unit factor(s) should we apply?
Since mol K = 6.02 10
23atoms K, the two unit factors are 1 mol K/6.02 10 23
atoms K, and its reciprocal 6.02 10 23
atoms K/1 mol K.
Unit Analysis Map
© 2011 Pearson Education, Inc.Introductory Chemistry: Concepts and Critical Thinking, 6th EditionCharles H. Corwin
Example Exercise 9.3Mole Calculations I
We apply the unit factor 1 mol K/6.0210
23atoms K to cancel atoms , which appears in the denominator.
The answer is rounded to three digits because the given value and unit factor each have three significant digits.
Solution
Calculate the number of moles of potassium iodide in 5.3410 25formula units of KI.
Answer:88.7 mol KI
Practice Exercise
What is the number of molecules in 1.00 mol of iodine crystals?Answer:See Appendix G.
Concept Exercise
Continued
© 2011 Pearson Education, Inc.Introductory Chemistry: Concepts and Critical Thinking, 6th EditionCharles H. Corwin
Example Exercise 9.4Molar Mass Calculations
We begin by finding the atomic mass of each element in the periodic table. The molar mass equals the sum of the atomic
masses expressed in g/mol. (a)The atomic mass of Ag is 107.87 amu, and the molar mass of silver equals 107.87 g/mol. (b)The sum of the atomic masses for NH 3 is 14.01 amu + 3(1.01)amu = 17.04 amu. The molar mass of ammonia equals 17.04 g/mol. (c)The sum of the atomic masses for Mg(NO 3 2 is