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Chemistry is the branch of science that studies the properties and behavior of matter, the changes it undergoes during chemical reactions, and the energy that accompanies those processes.

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• Label Parts of the Atom [ Google Apps worksheet ][ worksheet PDF ][ worksheet PNG ][ answers PNG ]
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Periodic Tables

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• Muted color 118 element periodic table [ PDF ]
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The starting materials consist of one green sphere and two purple spheres. The products consist of two green spheres and two purple spheres. This violates Dalton’s postulate that that atoms are not created during a chemical change, but are merely redistributed.

This statement violates Dalton’s fourth postulate: In a given compound, the numbers of atoms of each type (and thus also the percentage) always have the same ratio.

Dalton originally thought that all atoms of a particular element had identical properties, including mass. Thus, the concept of isotopes, in which an element has different masses, was a violation of the original idea. To account for the existence of isotopes, the second postulate of his atomic theory was modified to state that atoms of the same element must have identical chemical properties.

Both are subatomic particles that reside in an atom’s nucleus. Both have approximately the same mass. Protons are positively charged, whereas neutrons are uncharged.

(a) The Rutherford atom has a small, positively charged nucleus, so most α particles will pass through empty space far from the nucleus and be undeflected. Those α particles that pass near the nucleus will be deflected from their paths due to positive-positive repulsion. The more directly toward the nucleus the α particles are headed, the larger the deflection angle will be. (b) Higher-energy α particles that pass near the nucleus will still undergo deflection, but the faster they travel, the less the expected angle of deflection. (c) If the nucleus is smaller, the positive charge is smaller and the expected deflections are smaller—both in terms of how closely the α particles pass by the nucleus undeflected and the angle of deflection. If the nucleus is larger, the positive charge is larger and the expected deflections are larger—more α particles will be deflected, and the deflection angles will be larger. (d) The paths followed by the α particles match the predictions from (a), (b), and (c).

(a) 133 Cs + ; (b) 127 I − ; (c) 31 P 3− ; (d) 57 Co 3+

(a) Carbon-12, 12 C; (b) This atom contains six protons and six neutrons. There are six electrons in a neutral 12 C atom. The net charge of such a neutral atom is zero, and the mass number is 12. (c) The preceding answers are correct. (d) The atom will be stable since C-12 is a stable isotope of carbon. (e) The preceding answer is correct. Other answers for this exercise are possible if a different element of isotope is chosen.

(a) Lithium-6 contains three protons, three neutrons, and three electrons. The isotope symbol is 6 Li or 3 6 Li . 3 6 Li . (b) 6 Li + or 3 6 Li + 3 6 Li +

(a) Iron, 26 protons, 24 electrons, and 32 neutrons; (b) iodine, 53 protons, 54 electrons, and 74 neutrons

(a) 3 protons, 3 electrons, 4 neutrons; (b) 52 protons, 52 electrons, 73 neutrons; (c) 47 protons, 47 electrons, 62 neutrons; (d) 7 protons, 7 electrons, 8 neutrons; (e) 15 protons, 15 electrons, 16 neutrons

Let us use neon as an example. Since there are three isotopes, there is no way to be sure to accurately predict the abundances to make the total of 20.18 amu average atomic mass. Let us guess that the abundances are 9% Ne-22, 91% Ne-20, and only a trace of Ne-21. The average mass would be 20.18 amu. Checking the nature’s mix of isotopes shows that the abundances are 90.48% Ne-20, 9.25% Ne-22, and 0.27% Ne-21, so our guessed amounts have to be slightly adjusted.

Turkey source: 20.3% (of 10.0129 amu isotope); US source: 19.1% (of 10.0129 amu isotope)

The symbol for the element oxygen, O, represents both the element and one atom of oxygen. A molecule of oxygen, O 2 , contains two oxygen atoms; the subscript 2 in the formula must be used to distinguish the diatomic molecule from two single oxygen atoms.

(a) molecular CO 2 , empirical CO 2 ; (b) molecular C 2 H 2 , empirical CH; (c) molecular C 2 H 4 , empirical CH 2 ; (d) molecular H 2 SO 4 , empirical H 2 SO 4

(a) C 4 H 5 N 2 O; (b) C 12 H 22 O 11 ; (c) HO; (d) CH 2 O; (e) C 3 H 4 O 3

(a) CH 2 O; (b) C 2 H 4 O

(a) ethanol

(b) methoxymethane, more commonly known as dimethyl ether

(c) These molecules have the same chemical composition (types and number of atoms) but different chemical structures. They are structural isomers.

Use the molecular formula to find the molar mass; to obtain the number of moles, divide the mass of compound by the molar mass of the compound expressed in grams.

Formic acid. Its formula has twice as many oxygen atoms as the other two compounds (one each). Therefore, 0.60 mol of formic acid would be equivalent to 1.20 mol of a compound containing a single oxygen atom.

The two masses have the same numerical value, but the units are different: The molecular mass is the mass of 1 molecule while the molar mass is the mass of 6.022 × × 10 23 molecules.

(a) 256.48 g/mol; (b) 72.150 g mol −1 ; (c) 378.103 g mol −1 ; (d) 58.080 g mol −1 ; (e) 180.158 g mol −1

(a) 197.382 g mol −1 ; (b) 257.163 g mol −1 ; (c) 194.193 g mol −1 ; (d) 60.056 g mol −1 ; (e) 306.464 g mol −1

(a) 0.819 g; (b) 307 g; (c) 0.23 g; (d) 1.235 × × 10 6 g (1235 kg); (e) 765 g

(a) 99.41 g; (b) 2.27 g; (c) 3.5 g; (d) 222 kg; (e) 160.1 g

(a) 9.60 g; (b) 19.2 g; (c) 28.8 g

zirconium: 2.038 × × 10 23 atoms; 30.87 g; silicon: 2.038 × × 10 23 atoms; 9.504 g; oxygen: 8.151 × × 10 23 atoms; 21.66 g

AlPO 4 : 1.000 mol or 26.98 g Al Al 2 Cl 6 : 1.994 mol or 53.74 g Al Al 2 S 3 : 3.00 mol or 80.94 g Al The Al 2 S 3 sample thus contains the greatest mass of Al.

3.113 × × 10 25 C atoms

0.865 servings, or about 1 serving.

20.0 g H 2 O represents the least number of molecules since it has the least number of moles.

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Access for free at https://openstax.org/books/chemistry-atoms-first-2e/pages/1-introduction

• Authors: Paul Flowers, Edward J. Neth, William R. Robinson, PhD, Klaus Theopold, Richard Langley
• Publisher/website: OpenStax
• Book title: Chemistry: Atoms First 2e
• Publication date: Feb 14, 2019
• Location: Houston, Texas
• Book URL: https://openstax.org/books/chemistry-atoms-first-2e/pages/1-introduction
• Section URL: https://openstax.org/books/chemistry-atoms-first-2e/pages/chapter-2

© Jan 8, 2024 OpenStax. Textbook content produced by OpenStax is licensed under a Creative Commons Attribution License . The OpenStax name, OpenStax logo, OpenStax book covers, OpenStax CNX name, and OpenStax CNX logo are not subject to the Creative Commons license and may not be reproduced without the prior and express written consent of Rice University.

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2.15: Assignment—Atoms, Molecules, and Ions

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To download a copy of the assignment, please click on the link Sample Questions .

As you work these matter and measurement problems, consider and explain:

• What type of question is it?
• How do you know what type of question it is?
• What information are you looking for?
• What information do they give?
• How will you go about solving this?
• Show how to solve the problem.
• Be able to answer for a different reaction, number, set of conditions, etc.

Sample Questions

• NH 4 and NH 4 Cl
• ZnO 2 and ZnCl 2
• H 2 O and HCl
• NO and NO 2
• CH 4 and CO 2
• A sample of chemical X is found to contain 5.0 grams of oxygen, 10.0 grams of carbon, and 20.0 grams of nitrogen. The law of definite proportion would predict that a 70 gram sample of chemical X should contain how many grams of carbon?
• All atoms of the same element are identical.
• Compounds are combinations of different atoms.
• A chemical reaction changes the way atoms are grouped together.
• Atoms are indestructible.
• Who was the first scientist to show that atoms emit any negative particles?
• The Rutherford experiment proved the Thomson “plum-pudding” model of the atom to be essentially correct.
• The Rutherford experiment was useful in determining the nuclear charge on the atom.
• Millikan’s oil-drop experiment showed that the charge on any particle was a simple multiple of the charge on the electron.
• The electric discharge tube proved that electrons have a negative charge.
• All of the above experiments gave the results described.
• An atom is mostly empty space.
• Almost all of the mass of the atom is concentrated in the nucleus.
• The protons and neutrons in the nucleus are very tightly packed.
• The number of protons and neutrons is always the same in the neutral atom.
• All of the above statements (A–D) are true.
• The element rhenium (Re) exists as two stable isotopes and 18 unstable isotopes. What does Rhenium-185 have in its nucleus?
• 20 protons and 20 neutrons
• 21 protons and 19 neutrons
• 22 neutrons and 18 protons
• 20 protons and 22 neutrons
• 21 protons and 20 neutrons
• There is twice as much mass of hydrogen as oxygen in each molecule.
• There are two hydrogen atoms and one oxygen atom per water molecule.
• There is twice as much mass of oxygen as hydrogen in each molecule.
• There are two oxygen atoms and one hydrogen atom per water molecule.
• None of these.
• K, alkali metal
• Ba, alkaline earth metal
• Ne, noble gas
• Ni, transition metal
• Calcium, Ca
• good conductors of heat
• often lustrous
• tend to gain electrons in chemical reactions
• cobalt(II) chloride
• magnesium oxide
• aluminum(III) oxide
• diphosphorus pentoxide
• All of the above names are correct
• iodine trichloride, ICl 3
• phosophorus pentoxide, P 2 O 5
• ammonia, NH 3
• sulfur hexafluoride, SF 6
• All of the above pairs are correct.
• How many oxygen atoms are there in one formula unit of Ca 2+ ?
• What is the correct name for FeO?
• What is the correct name for Ca 2+ ?
• What is the correct name for V 3+ ?
• What is the subscript of barium in the formula of barium sulfate?
• What is the formula for calcium bisulfate?
• Pb(NO 3 ) 2 , lead(II) nitrate
• NH 4 ClO 4 , ammonium perchlorate
• PO 4 3− , phosphate ion
• Mg(OH) 2 , magnesium hydroxide
• NO 3− , nitrite ion

[reveal-answer q=”279540″]Show Sample Answers[/reveal-answer] [hidden-answer a=”279540″]

• J. J. Thomson
• 75 protons, 110 neutrons
• I, IV and II, V
• 20 protons, 20 neutrons, and 18 electrons
• 19 p, 20 n, 18 e
• iron(II) oxide
• calcium ion
• vanadium(III) ion
• Ca(HSO 4 ) 2

[/hidden-answer]

• Authored by : Jessica Garber. Provided by : Tidewater Community College. License : CC BY: Attribution

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Chemistry 10th Edition Whitten, Kenneth W.; Davis, Raymond E.; Peck, Larry; Stanley, George G.

Chemistry (12th edition) wilbraham, chemistry 12th edition chang, raymond; goldsby, kenneth, chemistry (4th edition) burdge, julia, chemistry (7th edition) mcmurry, john e.; fay, robert c.; robinson, jill kirsten, chemistry 9th edition zumdahl, steven s.; zumdahl, susan a., chemistry: a molecular approach (3rd edition) tro, nivaldo j., chemistry: an atoms-focused approach gilbert, thomas r.; kirss, rein v.; foster, natalie, chemistry and chemical reactivity (9th edition) kotz, john c.; treichel, paul m.; townsend, john r.; treichel, david a., chemistry: an introduction to general, organic, and biological chemistry (12th edition) timberlake, karen c., chemistry: atoms first (2nd edition) zumdahl, steven s.; zumdahl, susan a., chemistry: molecular approach (4th edition) tro, nivaldo j., chemistry: the molecular science (5th edition) moore, john w.; stanitski, conrad l., chemistry: principles and practice (3rd edition) reger, daniel l.; goode, scott r.; ball, david w., chemistry: the central science (13th edition) brown, theodore e.; lemay, h. eugene; bursten, bruce e.; murphy, catherine; woodward, patrick; stoltzfus, matthew e., chemistry: the molecular nature of matter and change 7th edition silberberg, martin; amateis, patricia, chemistry: the science in context (4th edition) gilbert, thomas r.; kirss, rein v., general chemistry (4th edition) mcquarrie, donald a., general chemistry 10th edition ebbing, darrell; gammon, steven d., general chemistry: principles and modern applications (10th edition) petrucci, ralph h.; herring, f. geoffrey; madura, jeffry d.; bissonnette, carey, general, organic, and biological chemistry: structures of life (5th edition) timberlake, karen c., general, organic, & biological chemistry 3rd edition smith, janice, introductory chemistry (5th edition) tro, nivaldo j., organic chemistry, 5th edition smith, janice, organic chemistry (8th edition) wade jr., l. g., organic chemistry 9th edition mcmurry, john e., organic chemistry as a second language, 3e: first semester topics klein, david, physical chemistry: thermodynamics, structure, and change atkins, peter; de paula, julio.

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Draw the Lewis structure of (CHO)OCH₃ and then choose the appropriate set of molecular geometries of the three central atoms. Your answer choice is independent of the orientation of your drawn structure.

The solubility of He in water at 25.0 °C is 7.0 × 10⁻⁵ M when the partial pressure of He is 0.20 atm. What is the value of the Henry's law constant for He ?

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According to the balanced reaction below, calculate the moles of NH₃ that form when 4.2 mol of N₂H₄ completely reacts 3 N₂H₄(l) → 4 NH₃(g) + N₂(g)

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What is the correct IUPAC name for HBrO(aq)?

What is the correct IUPAC name for Ca(BrO₂)₂?

What is the correct IUPAC name for Ti(ClO₄)₄?

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