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Chemistry Chapters 1,2,3 – Flashcards

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8 July 2022

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question

Which statement is true about matter? A.) Matter is particulate- it is composed of particles. B.) The structures of particles that compose matter determines the properties of matter. C.) The particles that compose matter include atoms and molecules. D.) All of the above statements are true

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All of the above statements are true.

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This image represents a particulate view of a sample of matter. Classify the sample according to its composition.

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The sample is a compound

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A chemist mixes sodium with water and witnesses a violent reaction between the two substances. This is best classified as a(n):

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Observation

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Two samples of a compound containing elements A and B are decomposed. The first sample produces 15 g A and 35 g B. The second sample produces 25 of A and what mass of B?

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58 g B

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A compound containing only only carbon and hydrogen has a carbon-to-hydrogen mass ratio of 11.89. Which carbon to hydrogen mass ratio is possible for another compound composed only of carbon and hydrogen?

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3.97

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Which concept was demonstrated by Rutherford's gold foil experiment?

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Atoms are mostly empty space.

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A student re-creates Millikan's oil drop experiment and tabulates the relative charges of the oil drops in terms of a constant, a. Drop 1-a Drop 2- 3/2 a Drop 3- 5/2 a Drop 4- 3 a

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1/2 a

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How many protons and neutrons are in the isotope Fe-58?

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26 protons and 32 neutrons

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An isotope of an element contains 82 protons and 122 neutron. What is the symbol of the isotope?

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204 Pb 82

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How many electrons are in the Cr3+ ion?

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21 electrons

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A naturally occurring sample of an element contains only two isotopes. The first isotope has a mass of 68.9255 amu and a natural abundance of 60.11%. The second isotope has a mass of 70.9247 amu. Determine the atomic mass of the element.

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69.72 amu

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Copper has an atomic mass of 63.55 amu and two naturally occurring isotopes with masses 62.94 amu and 64.93 amu. Which mass spectrum is most likely to correspond to a naturally occurring sample of copper.

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62.94 amu= 100% 64.93 amu= 45%

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All matter is composed of_

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particles

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The structure of the particles that compose matter determines the _ of matter

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properties

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_is the science that investigates the properties of matter by examining the atoms and molecules that compose matter it.

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Chemistry

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We classify matter according to its _ and _.

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state and composition

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Matter has three common states:__,__,and__.

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solid, liquid, and gas

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Matter can be __ or __

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pure substance or mixture

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A pure substance can be either a __ or __

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element or compound

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Mixture can be either __ or __

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heterogeneous or homogeneous

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Science begins with the __ of the physical world. A number of observations can often be summarized in a statement or generalization called a __.

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observation/ scientific law.

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A __ is a tentative interpretation or explanation of observation of observations. One or more well- established hypotheses may prompt the development of a scientific theory, a model for nature that explains the underlying reasons for observations and laws.

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hypothesis

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Laws, hypotheses, and theories all give rise to predictions that can be tested by __, carefully controlled procedures designed produce critical new observations. If scientists cannot confirm the predictions, they must modify or replace the law, hypothesis, or theory.

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Experiment

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Each element is composed of indestructible particles called__.

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atoms

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All atoms of a given element have the __ mass and other properties.

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same

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Atoms combine in simple, whole- number ratios to form__

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compounds

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Atoms of one element cannot change into atoms of another element. In a ___, atoms change the way that they are bound together with atoms to form a new substance.

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chemical reaction

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___discovered the electron in the late 1800s through experiments with cathode rays. He deduced that electrons are negatively charged, and he measured their charge-to-mass ratio.

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J.J. Thompson

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__ measured the charge of the electron, which-- in conjunction with Thompson's results- led to the calculation of the mass of an electron.

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Robert Millikan

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In 1909, ___ Ernest Rutherford probed the inner structure of the atom by working with a form of radioactivity called alpha radiation and developed the nuclear theory of the atom.

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Ernest Rutherford

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__ states that the atom is mainly empty space, with most of its mass concentrated in a tiny region called the nucleus and most of its volume occupied by relatively light electrons.

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Nuclear theory

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Atoms are composed of three fundamental particles__,__, and __

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protons, neutrons, and electrons

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The number of protons in the nucleus of the atom is its __. It determines the charge of the nucleus and defines the element.

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atomic number

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The __ tabulates all known elements in order of increasing atomic number.

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periodic table

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Atoms of an element that have different numbers of neutrons are __.

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isotopes

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Atoms that lose or gain electrons become charged and are called __. __ are positively charged and __ are negatively charged.

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ion/cation/anion

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Relationship between mass number, number of protons, and number of neutrons

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number of protons + number of neutrons

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atomic mass formula

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atomic mass= sigma (fraction of isotope n) x (mass of isotope n)

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What is the difference between a law and a theory?

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A law summarizes a series of related observations, while a theory gives the underlying reasons for them.

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When a log completely burns in a campfire, the mass of the ash is much less than the mass of the log. What happens to the matter that composed the log?

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Most of the matter that composed the log reacts with oxygen molecules in the air. The products of the reaction (mostly carbon dioxide and water) are released as gases into the air.

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Explain the difference between the law of definite proportions and law of multiple proportions.

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The law of definite proportions applies to two or more samples of the same compound and states that the ratio of one element to the other is always the same. The law of multiple proportions applies to two different compounds containing the same two elements (A and B) and states that the masses of B that combine with 1 g of A are always related to each other as a small whole- number ratio.

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Suppose that one of Millikan's oil drops has a charge of -4.8 x 10^-19 C. How many excess electrons does the drop contain?

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The drop contains 3 excess electrons (3 x (-1.6 x 10^-19 C)= -4.8 x 10^-19 C)

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In the light of the nuclear model for the atom, which statement is true?

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For a given element, the size of an atom is the same for all of the element's isotopes.

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Recall from the Conceptual Connection 1.6 that carbon has two naturally occurring isotopes C-12 (natural abundance is 98.93%; mass is 12.0000 amu) and C-13 (natural abundance is 1.07%; mass is 13.0034 amu). Without doing any calculations, determine which mass is closest to the atomic mass of carbon.

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12.0000 amu

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The density of copper decreases as temperature increases (as does the density of most substances). Describe the changes in a sample of copper when it is warmed from room temperature to 95 degrees C.

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The sample expands. However, because of its mass remains constant while its volume increases, its density decreases.

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Without doing any calculations, determine which sample contains the most atoms. A.) a 1-g sample of copper B.) a 1-g sample of carbon C.) a 10-g sample of uranium

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a 1-g sample of carbon.

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What is the mass of a 1.75-L sample of a liquid that has a density of 0.921 g/mL?

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1.61 10^3 g

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Convert 1,285 cm^2 to m^2

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0.1285 m^2

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Three samples, each of a different substance, are weighed and their volume is measured. The results are tabulated. List the substances in order of decreasing density. Substance 1- Mass 10.0 g. Volume 10.0 mL Substance 2- Mass 10.0 kg. Volume 12.0 L Substance 3- Mass 12.0 mg. Volume 10.0 ul

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3>1>2

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A solid metal sphere has a radius of 3.53 cm and a mass of 1.796 kg. What is the density of the metal in g/cm^3? The volume of a sphere is V= 4/3pi r^3

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3.6 mi/gal

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A German automobile's gas mileage is 22 kn/L. Convert this quantity to miles per gallon.

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1.13 cm^3

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A wooden block has a volume of 18.5 in^3. Express the volume of the cube in cm^3.

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14 g C

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Which sample contains the greatest amount of atoms? A.) 14 g C B.) 49 g Cr C.) 102 g Ag D.) 202 g Pb

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0.20 cm

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Determine the number of atoms in 1.85 mL of mercury. The density of mercury is 13.5 g/mL.

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7.50 x 10^22 atoms

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A 20.0- g sample of an element contains 4.95 x 10^23 atoms. Identify the element.

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question

Measurements usually involve the use of ___, which have an inherent amount of uncertainty.

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instruments

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In reported measurements, every digit is certain except the __, which is estimated. The ___ of a measurement refers to its reproducibility.

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last/ precision

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The __ of a measurement refers to how close a measurement is to the actual value of the quantity being measured.

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accuracy

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The __ of a substance is the ratio of its mass to its volume.

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density

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Density is a __ property, which means it is independent of the amount of substance.

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intensive

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__ is the capacity to do work and is often reported in units of ___. Systems with high potential energy tend to change in the direction of lower potential energy, ___ energy to its surroundings.

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Energy/joules/releasing

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In chemical and physical changes, matter often exchanges energy with its surroundings. In these exchanges, the total energy is always ___, energy is neither created nor destroyed.

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conserved

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A process in which a system transfers energy to the surroundings in ____. A process in which a system gains energy from the surroundings in ___.

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exothermic/endothermic

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____ solving problems by using units as a guide- is useful in solving many chemical problems.

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dimensional analysis

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Four steps in solving a chemical equation

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sort, strategize, solve, and check

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One __ of an element is the amount of that element that contains Avogadro's number of atoms.

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mole

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Any sample of an element with a mass that equals its atomic mass contains one __ of that element. Fore example, the atomic mass of carbon is 12.011 amu, therefore 12.011 g of carbon is 1 mol of carbon atoms.

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mole

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Density formula

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Density=mass/volume

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Avogadro's number

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1 mol= 6.0221421 x 10^23 particles

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Arrange the following types of electromagnetic radiation in order of (a) increasing frequency; and (b) increasing wavelength: visible, X-ray, infrared

answer

A.) infrared

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We shine light of three different wavelengths- 325 nm, 455 nm, and 632 nm- on a metal surface. The observation for each wavelength, labeled A, B, and C, are: Observation A: No photoelectrons are observed Observation B: Photoelectrons with a kinetic energy of 155 kJ/mol are observed. Observation C: Photoelectrons with a kinetic energy of 51 kJ/mol are observed. Which observation corresponds to which wavelength of light?

answer

Observation A- 632 nm. Observation B-325 nm. Observation C- 455 nm. The shortest wavelength of light (highest energy photon) corresponds to the photoelectrons with the greatest kinetic energy. The longest wavelength of light (lowest energy per photon) corresponds to the instance where no photoelectrons were observed.

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Since quantum- mechanical theory is universal, it applies to all objects, regardless of the size. Therefore, according to the de Broglie relation, a thrown baseball should also exhibit wave properties. Why don't we observe such properties at the ballpark?

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Because of the baseball's mass, its de Broglie wavelength is minuscule. This minuscule wavelength is insignificant compared to the size of the baseball itself, and therefore its effects are not observable.

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What values of l are possible for n=3? A.) 0 (or S) B.) 0 and 1 (or s and p) C.) 0,1,2 (or s,p, and d) D.) 0,1,2,and 3 (or s,p,d, and f)

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question

What values of ml are possible for l=2? A.) 0,1,2 B.)0 C.) -1,0,1 D.) -2,-1,0,1,2

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Which transition results in emitted light with the shortest wavelength? A.) n=5--> n=4 B.) n=4-->n=3 C.) n=3-->n=2

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Which wavelength of light has the highest frequency? A.) 10nm B.) 10mm C.) 1nm D.) 1mm

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Which kind of electromagnetic radiation contains the greatest energy per photon? A.) Microwaves B.) Gamma rays C.) X-rays D.) Visible light

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How much energy ( in J) is contained in 1.00 moles of 522-nm photons? A.) 3.60x10^-19J B.) 2.17x10^5J C.) 3.60x10^-28J D.) 5.98x10^-43J

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question

Light from three different lasers (A, B, C), each with a different wavelength, is shined into the same metal surface. Laser A produces no photoelectrons. Lasers B and C both produce photoelectrons, but the photoelectrons produced by Laser B have a greater velocity than those produced by Laser C. Arrange the lasers in order of increasing wavelength. A.) A

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question

Calculate the frequency of an electron traveling at 1.85x10^7 m/s A.) 1.31x10^-19 s^-1 B.) 1.18x10^-2 s^-1 C.) 3.93x10^-11 s^-1 D.) 7.63x10^18 s^-1

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Which set of three quantum numbers does not specify an orbital in the hydrogen atom? A.) n=2; l=1; ml=-1 B.) n=3; l=3; ml=-2 C.) n=2; l=0; ml=0 D.) n=3; l=2; ml=2

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question

Calculate the wavelength of light emitted when an electron to the hydrogen makes a transition from an orbital with n=5 to a orbital with n=3. A.) 1.28x10^-6 m B.) 6.04x10^-7 m C.) 2.28x10^-6 m D.) 1.55x10^-19 m

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Which electron transition produces light of the highest frequency in the hydrogen atom? A.) 5p--> 1s B.) 4p--> 1s C.) 3p--> 1s D.) 29--> 1s

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How much time (in seconds) does it take light to travel 1.00 billion km? A.) 3.00x10^17 s B.) 3.33 s C.) 3.33x10^3 s D.)3.00x10^20 s

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question

Which figure represents a d orbital?

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four petals

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The theory of ____ explains the behavior of absolutely small particles, such as electrons, in the atomic and subatomic realms.

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quantum mechanics

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These particles behave differently than the sorts of particles we see in the ___.

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macroscopic world

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Light is a type of ____- a form of energy embodied in oscillating electric and magnetic fields that travels through space at 3.00x10^8 m/s.

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electromagnetic radiation

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The wave nature of light is characterized by its___ the distance between wave crests-- and its ability to experience ___ and___.

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wavelength/interference/diffraction

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The ____ includes all wavelengths of electromagnetic radiation from gamma rays to radio waves. Visible light is a tiny sliver in the middle of this.

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electromagnetic spectrum

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The particle nature of light is characterized by _______.

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specific quantity of energy carried in each photon.

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___ is the study of light absorbed and emitted by atoms when an electron makes a transition from one energy level to another.

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Atomic spectroscopy

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The wavelengths absorbed or emitted depend on the energy differences between the levels involved in transition; large energy differences result in ___, and small energy differences result in___.

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short wavelength/long wavelength

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Electrons have a wave nature with an associated wavelength, as quantified by the____.

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de Broglie relation

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The wave nature and particle nature are ___- the more we know about one, the less we know of the other.

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complementary

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The wave- particle duality of electrons is quantified in ____, which states that there is a limit to how well we can know both the position of the electron and the velocity times the mass of an electron- the more accurately one measured, the greater uncertainty in measurement of the other.

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Heisenberg's uncertainty principle.

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The inability to simultaneously know both the position and the velocity of an electron results in ___, the inability to predict a trajectory for an electron. Consequently, electron behavior is described differently than the behavior of everyday- sized particles.

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indeterminacy

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The trajectory we normally associate with macroscopic objects in replaced, for electrons, with statistical descriptions that show, not the electron's path, but____.

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the region where it is most likely found.

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The most common way to describe electrons in atoms according to quantum mechanics is to solve the ___ for the energy states of the electrons within the atom. When the electron is in these states, its energy is well defined but its position is not. The position of an electron is described by a probability distribution map called an ___.

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Schrodinger equation/orbital

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The solutions to Schrodinger equation are characterized by quantum numbers:___.

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n,l and ml

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The ___ determines the energy of the electron and the size of the orbital; the ___ determines the shape of the orbital; the __ determines the orientation of the orbital. A fourth quantum number, the ___, specifies the orientation of the spin of the electron.

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principle quantum number/angular momentum quantum number/magnetic quantum number/spin quantum number.

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Relationship between Frequency (v), Wavelength (lambda), and the speed of light

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V=c/lambda

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Relationship between Energy (E), Frequency (v), Wavelength (lambda), and Planck's constant (h)

answer

E=hv E=hc/lambda

Chemistry Chapters 1,2,3 – Flashcards

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