Atomic Structure BFF: Homework Helper and Test Prep Guide for HS Chemistry

for

High School Chemistry This topic is from my book:

Surviving Chemistry BFF: Homework Helper and Test Prep Guide.

Teachers and students can get it in Hard Copy or Copy or ebook from

SurvivingChem.com or Amazon.com

Click here to get other oth er topics from TpT

7– 22 23– 34

35– 52 53– 70 71– 86

87– 102 103– 118

119– 132

133 – 152

153 – 170 171– 1– 192 193 – 212 213 – 220

221– 231

233 – 236

Copyright ©201 ©2014. E3 Schola cholastic Publishing Publishing.

SurvivingChem.com

5

 The basic unit of matter.

 Earliest model

 John Dalton No internal structure.

(cannonball) model

model

(nuclear) model

(planet (planetar ary) y) model model

 J.J. Thomson Electrons and positive charges disperse throughout the atom.

- + -- + +-+-+ -+-+-+

Ernest Ernest Rutherford Rutherford  A small and dense positive positive (+) nucleus. Most of atom is empty space. Electrons revolve around the nucleus.

Neils Bohr Electrons in specific orbit . Orbits have fixed energy. Orbits are the electron shells.

empty space

+

+

e-

orbit (electron shells)

 Work of many Scientists Scientists over hundreds of years.  The current model model of the atom. (electron-cloud) model Small, dense, positive nucleus. Protons Protons and neutrons in the nucleus. Electrons in orbital outside the nucleus.

+

Orbital current model Probable location of finding an electron ele ctron with a specific energy. Copyright © 2011. E3 Scholastic Publishing. SurvivingChem.com

35

8. J.J. J.J. Thoms Thomson: on:

 A cathode ray tube containing containing two metal disks was connected to the + and – ends of an electrical el ectrical source.  A positive (+) and negative (-) plates were placed placed above and below below the cathode cathode ray tube. Result 1 Conclusion 1

 A beam of light (ray) travels travels from the cathode cathode disk (-) to the anode disk (+).  The beam is composed composed of particles.

deflected toward the positive positive plate. Result 2  The beam was deflected beam are negatively charged charged (electrons). Conclusion 2   The particles in the beam 9. Ernest Rutherford:

The Setup

Result 1 Conclusion 1 Result 2

 were fired at a gold foil. foil.  A fluorescent screen screen detects paths of of the alpha alpha particles once they had hit the gold foil. Most particles went straight through the gold foil undeflected.  An atom is mostly empty empty space ( Empty Empty Space Theory )  Very few particles were were deflected straight back or at angles.

center of an atom is dense, dense, positive, and very small. Conclusion 2   The center

 36

 Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

 The inner core core of an atom. Dense, small, and positive. Contains the protons and neutrons.  Accounts for most of an atom’s mass.

nucleus

Protons(+)

Protons (+ charge)

Neutrons

Electrons (- charge) Neutrons (no charge)

Electrons (-)

+1 charge 1 atomic atomic mass unit (1 amu) Located in the nucleus 0 charge 1 amu Located in the nucleus -1 charge 0 mass ( 1/1836th of a proton’s mass) Located outside the nucleus in orbitals Identifies each element. element.  The same value as the number of protons. protons.  The overall charge of the the nucleus (+).  The same value as the number of protons protons (or the atomic number). Identifies isotopes of an element.  The sum of protons protons plus neutrons. neutrons.  Particles in the nucleus. Protons and neutrons. Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

37

 Atoms of the same element. element. • Same number number of protons protons (same atomic #) • Different numbers of neutrons (different mass #’s)

Nuclide names Nuclide symbols Mass Numbers (different)

Isotope notations

 Atomic Number Number (same). (same). Number of Protons. # of Neutrons (different) (Mass# - Atomic #) #)

Nuclear diagrams

22.898

Na 23

11 p 12 n

11 p 13 n

 The average mass of an element’s naturally naturally occurring isotopes. Can be be found found on the the Period Periodic ic Table Table or Can be calculated from mass numbers and  percent  percent  an element’s natural isotope is otopes. s. abundances of  an

1 amu = 1/12th the mass of Carbon–12  3rd shell

Energy levels of an a n atom.

2nd shell 1st shell

 Atomic model of an element element that shows all the electron shells. Bohr’s diagram for Sodium (Na) is shown on the right.  The arrangement arrangement of electrons in the electron shells of an atom.  38

 Copyright © 2014. E3 Scholastic Publishing.

2 e8 e1 e-

2 – 8 – 1 1st

# of e-

2nd 3rd

SurvivingChem.com

shell

Key Concept

Definitions Definitions and facts

Examples

 The lowest energy and most stable state of of an atom. Electrons are in order from lowest to highest shell. s hell. Ground state electron configurations are given on the Periodic Table. For sodium sodium (Na): (Na): 2 – 8 – 1  The high energy and unstable state of an atom. Electrons are not in order. Excited state electron configuration of an atom is differen differentt from what what is given on the Periodic Table. For sodium sodium (Na): (Na): 2 – 7 – 2 (may vary, but the total e- must be 11)  An electron can move from one one shell to another depending if energy is absorbed or released.

2nd

rd

rd

nd

3

(Bright-line Spectrum)

From low (ground) state state to high (excited) (excited) state:  The electron absorbs absorbs energy From high (excited) state to low (ground) state:  The electron releases energy Band of colors produced when an excited electron releases energy as it returns from from a high to to low state. nd shell  The electron transition from from 3rd shell  will produce bright-line spectrum. spectrum. Shows line of colors produced at specific wavelengths Pattern of colors is unique for f or each element, and can be for for identificat identification. ion.  wavelength (nm) I

I

I

I

I

I

H Li Na Unknown

 The unknown sample sample contains H and and Na.

 A lab procedure in which compounds compounds of metallic ions are heated to produce unique u nique flame colors (light energy). It can be used to make mak e a rough identification of the metallic ion that is present in a sample. Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

39

Key Concept

Sulfur

Definition Definition and facts

2–8–6

Key examples

Electrons in the outermost level of an atom.  The last number in number in a configuration is always the number of valence electrons (for sulfur: s ulfur: 6 ).  A neutral atom may lose or share its valence valence e-, or gain e- to fill up its i ts valance shell during bonding.  Atoms with equal number of protons protons to electrons.  A neutral S atom has: 16 protons protons (+) 16 electrons (–) Charged atoms with unequal u nequal numbers of protons to electrons.

Formed by a neutral (metal) atom losing e-.

Na atom

Na+ ion

11+ 2 8 1

11+ 2 8

11+ protons 11+ 11 e- electrons 10 e2–8–1 electron 2–8 configurations

Na+ ion is formed when Na atom (a metal) loses 1 electron.

 A +ion always has fewer e- than the the atom. Na+ has 1 fewer electron than Na atom.

 A +ion always has more protons protons than electrons. electrons. Na+ has more protons (11+) than electrons (10e-).

 A +ion is always smaller than the atom. Na+ is smaller than Na atom.

Formed by a neutral (nonmetal) (nonmetal) atom gaining e-. S atom

S

2-

ion

S2- ion is formed when S atom (a nonmetal) gains 2 electrons.

 A – ion ion always has more e- than the atom. 16+ 2 8 6

16+ 2 8 8

S2- has 2 more electrons than S atom.

 A –ion always has fewer protons protons than electrons. 16+ protons 16+ 16 e- electrons 18 e2–8–6 electron electron 2–8–8 configurations

 40

S2- has fewer protons (16+) than electrons (18e-).

 A –ion is always larger than the atom. atom. S2- is larger than S atom. a tom.

 Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

To find

Key relationships

Examples

= atomic # of the element = # of electro electrons ns (in a neutral neutral atom) atom) = = nucleon – neutrons = mass # – neutrons = = protons (in neutral atoms) = nuclear charge = mass # – neutrons

(in ions)

 An atom with a +30 and 33 neutrons has 30 protons.

 A neutral atom of of has 35 electrons.

= atomic # charge of the ion = = nuclear charge – charge of the ion

 A charged atom  with and has 42 electrons

=m = mass # – atomic # = mass # – electrons (in neutral atoms) = nucleons – protons

 An atom with a

= protons = electrons (in neutral atoms) = nuclear charge =

 An atom with a

has 125 neutrons.

and has an atomic # of 52. The atom is tellurium.

 An atom with = neutrons + protons and =  ) ( neutral neutral atoms  has a = nuclear charge + neutrons mass # of 122 amu. = nucleons = mass # = protons + neutrons = neutrons neutrons + electrons = nuclear charge + neutrons

 An atom with a

= protons

 An atom of argon  with a mass of 40 40 amu has a nuclear charge of

= electron (in neutral atom) = mass # neutrons Copyright © 2014. E3 Scholastic Publishing Publishing..

SurvivingChem.com

65 neutrons has a total of 113 nucleons.

41

 protons = atomic number num ber = nuclear cha rge = electrons = mass # - neutrons = nucleo ns - neutrons

mass # = nucleons nucleons = protons protons + neutrons = nuclear charge + neutrons = electrons electrons + neutrons

neutrons = mass # - protons

= nucleons nu cleons – protons

 Atomic mass is the calculated average mass of all of an element’s element’s naturally occurring isotopes.  An example problem and solution (steps (steps and setup) for calculating an atomic atomic mass is given below.  A sample of an unknown element, X, contains contains the following isotopes: isotopes: 80 % of 64X, 15% of 65X, and 5% of 66X.  What is the average atomic mass of element X?

Step 1

Step 2

Step 3

(% to decimal) x (mass #) =

80% of

64X

.80

x

64

=

Step 4

(product)

51.2 +

15% of

65X

.15

x

65

=

9.75 +

5% of

66X.

.05

(.80)(64)

 42

x

+

66

(.15)(65)

=

+

(add all products)

3.3

(.05)(66) =

 Copyright © 2014. E3 Scholastic Publishing.

= 64.25 amu  atomic mass of X

 64.25 amu

SurvivingChem.com

Questions for Regents Practice Parts A and B-1

Atomic Structure Multiple Choice

1. Which conclusio conclusion n was a direct result of the the gold foil foil experim experiment? ent? 1) An ato atom is com composed of at leas east thr three types ypes of suba subattomic part partiicles cles.. 2) An atom is mostly mostly empty space space with a dense, positively positively charged charged nucleus. 3) An electron electron has a positive charge and is located inside the nucleus. nucleus. 4) An electron electron has has properties properties of of both waves waves and particles particles.. 2. In the wave-mechan wave-mechanical ical model of the atom, orbitals orbitals are regions regions of the most probable locations of  1) protons 2) positrons 3) ne neutrons 4) electrons 3. What is is the charge charge and mass mass of an an electron? electron? 1) Charg hargee of of +1 and and a mass mass of 1 am amu 3) Charge arge of +1 and and a mas masss of of 1/1 1/18836 amu 2) Charge of -1 and a mas mass of of 1 amu 4) Charge of -1 and a mas mass of of 1/18 /1836 amu

4. Which phrase phrase describes describes an atom? atom? 1) a positivel positivelyy charged charged electron electron cloud cloud surrounding surrounding a positiv positively ely charged charged nucleus nucleus 2) a positivel positivelyy charged charged electron electron cloud cloud surrounding surrounding a negativ negatively ely charged charged nucleus nucleus 3) a negatively negatively charged electron electron cloud surrounding a positively positively charged charged nucleus 4) a negatively negatively charged electron electron cloud surrounding a negatively negatively charged charged nucleus nucleus 5. Which total total mass mass is the the small smallest? est? 1) the the mass mass of of 2 elect electron ronss 2) the the mass mass of of 2 neutr neutrons ons 3) the mass mass of 1 electron electron plus plus the mass mass of 1 proto proton n 4) the mass mass of 1 neutron neutron plus plus the mass mass of of 1 electron electron 6. Which statement statement concerning elements elements is true? true? 1) Different elements must have have different numbers of isotopes. 2) Different elements must have have different numbers of neutrons. neutrons. 3) All atoms atoms of a given element must must have have the same mass number. number. 4) All atoms atoms of a given element must must have have the same atomic number. 7. Which value of an element element is calculated calculated using both the the mass and the the relative abundance of each of the naturally occurring isotopes of this element? 1) Atomic number 2) Atomic mass 3) Half-life 4) Molar volume 8. Which sequence sequence represents a correct order order of historical historical developments developments leading to the modern model of the atom? 1) Atom is a hard sphere atom is mostly empty space electrons exist in orbitals outside the nucleus 2) Atom is a hard sphere electrons exist in orbitals outside the nucleus atom is mostly empty space 3) Atom is mostly empty space atom is a hard sphere electrons exist in orbitals outside the nucleus 4) Atom Atom is empty empty space space electrons electrons exist in orbitals orbitals outside outside the nucleus nucleus atom is a hard sphere 9. An atom is electrica electrically lly neutral neutral because because the 1) number number of proton protonss equals the the number of of electrons electrons 2) number number of proton protonss equals the the number of of neutrons neutrons 3) ratio of of the number number of neutron neutronss to the numb number er of electro electrons ns is 1:1 4) ratio of of the number number of neutron neutronss to the the number number of proton protonss is 2:1 Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

43

Questions for Regents Practice: Parts A and B-1

Atomic Structure Multiple Choice

10. How do the energy energy and the most probable probable location of an electron in the the third shell of an atom compare to the energy and the most probable location of an  electron in the first shell of the same atom? 1) In the third shell, an electron has more more energy and is closer to the the nucleus. 2) In the third shell, an electron has more more energy and is farther from the nucleus. 3) In the third third shell, an electron has less energy and and is closer closer to the nucleus. 4) In the third shell, an electron has less energy energy and is farther farther from the the nucleus. 11. During a flame flame test, ions of a specific metal are heated heated in the flame of of a gas burner. A characteristic color of light is emitted by these ions in the flame  when the electrons electrons 1) gain energy energy as they they return return to lower lower energy energy levels 2) gain energy energy as they they move move to higher higher energy energy levels levels 3) emit energy energy as they they return return to lower lower energy energy levels levels 4) emit energy energy as they they move move to higher higher energ energyy levels 12. A particle of an atom contains contains 26 protons, 23 electrons, and 56 neutrons.  What will be the correct atomic atomic number for this particle? particle? 1 ) 26 2) 23 3) 56 4 ) 33 13. An atom atom with 21 neutrons and 40 nucleons has 1) A nuclear charge of +19 3) A mass number of 61 2) A nuclear charge of +40 4) A mass number of 19 14. Which element could could have a mass number of 86 atomic mass mass units and 49 neutrons in its nucleus? 1) In 2) Rb 3 ) Rn 4) Au 15. Which corre correctly ctly represents represents two isotopes isotopes of element element X? 1) 226 X and 226 X 3) 227 X and 91

2)

226

91

X and

91

91

227 X

4)

91

90

X and

90

16. Which atom atom is an isotope of oxygen? 14 1)  N 2) 16 N 7

226

8

3)

227 X 

227 X 

91

14 O

4)

7

17. What What is the total total number number of nucleons nucleons in the the nuclide nuclide

17O

8 65 Zn? 30

1) 65

2) 30

3) 35

4) 95

18. In which pair of atoms do the nuclei contain the the same number of neutrons? neutrons? 1) Calcium-40 and Calcium-42 3) Bromine-83 and Krypton-83 2) Chlorine-35 an and Su Sulfur-34 4) Iodine-127 and Bromine-80

 44

 Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

Questions for Regents Practice: Parts A and B-1

Atomic Structure Multiple Choice

19. Which is a ground state state electron configuration of of an atom in the fourth period period of the periodic table 1) 2 – 8 – 4 3) 2 – 8 – 18 – 18 – 4 2) 2 – 8 – 18 – 4 4) 2 – 4 20. The total total number of electrons found in the electron electron configuration configuration of a neutral chromium atom is 1 ) 24 2) 6 3) 13 4) 52 21. The highest amount of energy will will be emitted by an electron when it moves from the 1) 4th to 1st el  electron shell 3) 1st to 5th electron shell 2) 1st to 4th el  electron shell 4) 5th to 4th electron shell 22. What is the the total number number of electrons in a Cr3+ ion? 1) 3 2) 21 3) 24

4) 27

23. Which symbol represents a particle with with a total of 10 electrons? electrons? 3+ 1) N 2) Al 3) N 4) Al 3+ 24. Which electron configuration represents an atom atom of aluminum aluminum in an excited state? 1) 2-7-4 2) 2-8-3 3) 2-7-7 4) 2-8-6 25. Element X has two isotopes. isotopes. If 72.0% of the element has an isotopic isotopic mass of  84.9 amu, and 28.0% of the element has an isotopic mass of 87.0 amu, the average atomic mass of element X is numerically equal to 1) (72.0 + 84 84.9) x (28.0 + 87.0)

(72.0 x 84.9) (28.0 x 87.0) 3) ------------------ + ------------------100 100

2) (72.0 - 84.9) x (28.0 + 87.0)

(72.0 x 84.9) 4) ----------------100

(28.0 x 87.0) - -----------------100

26. The diagram below below represents represents the nucleus of of an atom

 What are the atomic atomic number and mass mass number of this atom? 1) The atomic atomic number is 9 and the the mass number is 19. 2) The atomic atomic number is 9 and the the mass number is 20. 3) The atomic atomic number is 11 and the the mass number is 19. 4) The atomic atomic number is 11 and the the mass number is 20.

Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

45

Questions for Regents Practice: Parts B-2 and C

Atomic Structure Constructed Constructed Response Response

27. Based on the atomic atomic mass and the natural natural abundances shown shown in the data table show a correct numerical numerical set-up for calculating the average atomic atomic mass of neon. 28. Based on natural abundances, abundances, the average atomic atomic mass of neon is closest closest to  which whole whole number? 29. In terms of atomic atomic particles, state state one difference between these these three isotopes isotopes of neon.

30. Explain, in terms of excited state, energy transitions, transitions, and ground ground state, how a bright-line spectrum is produced. 31. Identify Identify the two two elements elements in in the unknown unknown spectrum spectrum..

32. Write an appropriate appropriate number of electrons electrons in each shell to represent represent an Mg-26 atom in an excited state. Your Your answer may include include additional additional shells. 33. What is the total number number of valence electrons in an atom of Mg-26 Mg-26 in the ground state?

 46

 Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

Uses a set of four quantum numbers to describe location and behavior of an electron in atoms.

Principal Energy Level (n)

1,2,3.. or K, L, M.. are used to designate the major energy level of an a n electron. electron.  An electron electron with a first quantum level number of 2 or L is in the second energy s, p, d, f... are used us ed to indicate the sublevel of an electron within a principal energy level.

Sublevel of an Electron number of electrons sublevel  principal energy level le vel

 The difference between between the sublevels is the shape of their orbitals. s sublevel is always the first in any principal energy level. s sublevels sublevels have spherical spherical shape. shape. p sublevel is always next in any level. p sublevels have dumbbe dumbbell-like ll-like shape shape Shapes of d, f, g and h sublevels are too complex, and will not be discussed here.

Orbital (Probable Location)

x, y and z are used too describe the the orbital (probable location) of an electron within a sublevel. 2px, 2py , and 2pz describe the three p orbitals of of the second energy level. s sublevels sublev els (regardless of the energy level) have 1 orbital. p sublevels sublevels have 3 orbitals. orbitals. d sublevels have 5 orbitals. Each orbital, orbital, regardless regardless of the sublevel, sublevel, can hold a maximum of two electrons.

Spin Direction of an Electron

In full orbitals, orbitals, the two two electrons electrons must spin in opposite directions to overcome like-charge repulsion.

Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

47

Ground state atoms have configurations that show completely filled lowest available sublevels lowest energy

increasing energy---energy------------> -------->

Shows arrangement of electrons in the energy levels and sublevels. all lowest sublevels have their maximum maximum # of of electrons.

Ground State for Na

the 2p sublevel is incomplete while 3s has an extra electron

Excited State for Na

Shows distribution of of electrons electrons in the orbitals.

Ground state orbital notation notationss and electron electron configurations for four atoms are shown below.

H 1 e-

1s1

He 2 e-

1s2

 When placing electrons electrons in orbitals: No more than two electrons in an orbital Each orbital in p, d, f..etc must mu st have an electron before pairing  Two electrons in an orbital orbital must show opposite spins (  Valence electrons electrons are only  the  the electrons in the s and p sublevels of the highest level.

N

 48

7 e-

1s2

2s2

2p3

S 16 e-

1s2

2s2

2p6

 Copyright © 2014. E3 Scholastic Publishing.

3s2

3p4

SurvivingChem.com

Principal Energy Level (n) 1

Number of Sublevels 1

 2

2

3

3

4

4

 vailable Sublevels

Number of  aximum number of  Orbitals electrons in energy level  vailable (2n2) 1s 1 2 2s  1 8 2 3 3s  1 3p 3  18 3d 5 4s 1 4p 3 32 4d 5 4f 7 Note: Each orbital orbital can hold hold a maximum of 2 electrons electrons

34. What is the total number number of occupied occupied energy levels in an atom atom of neon in the ground state? 1) 1 3) 8 4) 18 2) 2  35. Which of the the followin followingg subleve sublevels ls has the the highest highest energy? energy? 1 ) 2p 2) 3p 3) 3d 4) 4s 36. What is the maximum maximum number number of electrons that can be be found in a 3s orbital of a potassium atom? 1) 1 2) 2 3) 8 4) 18 37. Which is the correct electron configuration of a magnesium magnesium atom atom in the ground state? 1) 1s2 2s2 2p6 3s1 3p1 3) 1s2 2s2 2p6 3s2 2) 1s2 2s2 2p6 4) 1s2 2s2 2p6 3s2 3p1

38. An atom atom in the excited state can have an electron electron configuration configuration of  1)1s2 2p1

2) 1s2 2s2

3) 1s2 2s2 2p5

4) 1s2 2s2 2p6

39. What is the electron electron configuration configuration of an Mn atom in the excited excited state? 1) 1s2 2s2 2p6 3s2 2) 1s2 2s2 2p6 3s2 3p6 3d6 4s1

3) 1s2 2s2 2p6 3s2 3p6 3d54s2 4) 1s2 2s2 2p6 3s2 3p6 3d5

40. Which atom in the ground state has only three electrons in the 3p sublevel? sublevel? 1) Ph Phosphorus 2) Po Potassium 3) Ar Argon 4) Al Aluminum 41. Which atom in the ground state has has two half-filled orbitals? orbitals? 1) P 2) O 3) Li 4) Si 42. What is the total number number of completely completely filled principal energy levels in an atom 2  with a configuration configuration of 1s 2s2 2p6 3s2 3p6 3d10 4s2 4p1 ? 1) 1 2) 2 3) 3 4) 4 43. Using quantum method ( s, p, d..), write electron configurations and and draw orbital notations for the following atoms and ions.

atoms: atoms: C, Al, S, Ar, Ca, Se

Copyright © 2014. E3 Scholastic Publishing.

ions: Li+, Mg 2+, K +, F-, S2-, As3SurvivingChem.com

49

Energy of an electron electron is quantized, meaning, it is specific specific for each energy level.  The equation below can be used to calculate the energy, En , of an electron in a hydrogen atom if its  principal energy energy level, n, is known. -2.178 x 10-18  En  = ----------------------------------- Joules Joules 2 n

c  = -----

electromagnetic radiation that Light is a form of electromagnetic travels at a of 3.00 x 108 m/sec. Every electromagnetic radiation (different light colors) is emitted at a specific (  ). Hertz, indicates the Frequency ( ) of light, in Hertz, number of completed wave per second. s econd.

/;  When an atom absorb or or release energy in the form of electromagnetic electromagnetic radiation during electron electron transition transition = h = -----from one energy level to another, the energy energy change change,, (in Joules), can be calculated using this equation. = Planck’s constant, 6.63 x 10-34  Joules.sec. = frequency of of the radiation (1/sec or Hz) = wavelength of the radiation (m) = speed of light, light, 3.00 x 108 m/sec 44. Calculate the energy energy of an electron of of a hydrogen hydrogen atom in these three three shells. a) n = 1 b) n= 2 c) n = 3 45. Violet light light has a wavelength of 4.10 4.10 x 10-12 m. What is its frequency? 46. A helium laser emits light with a wavelength of of 633 nm. What is the the frequency of  of  the light? 47. Calculate the wavelength wavelength of radiation with a frequency of 8.0 8.0 x 1014 Hz. 48. Green light light has a frequency of 6.01 6.01 x 1014 Hz. What is the wavelength? 49. Calculate the energy of a photon photon of radiation radiation with a frequency of 8.5 x 1014 Hz. 50. Calculate the energy of a gamma ray photon photon whose frequency frequency is 5.02 x 1020 Hz. 51. Calculate the energy of a photon photon of radiation radiation with a wavelength wavelength of 6.4 x 10-7 m. 52. What is the energy energy of light whose wavelength wavelength is 4.06 x 10-11 m? 53. An FM radio radio station broadcasts at a frequency of 107.9 MHz. MHz. What is the  wavelength of of the radio signal?

 50

 Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

Copyright © 2014. E3 Scholastic Publishing Publishing..

SurvivingChem.com

51

Questions for Regents Practice

 Answers

Atomic Structure  Topic 3

1. 2

14. 2

2. 4

15. 2

3. 4

16. 4

4. 3

17. 1

5. 1

18. 2

29. They contain different number of neutrons.

6. 4

19. 2

7. 1

20. 1

30. Spectrum is produced when produced  when excited e- returned to gro ground und state. state. (answer may vary)

8. 1

21. 1

9. 1

22. 2

10. 2

23. 4

11. 3

24. 1

12. 1

25. 3

13. 1

26. 2

27. (.909 x 20) + setup setup may vary vary 28. 20

31. He and H 32 2 – 8 – 1 – 1 or 2–7–3 (configuration may vary, BUT must have 12 electrons) 33. 2

 Additional Materials 34) 2 35) 3 36) 2 37) 3 38) 1 39) 2 40) 1 41) 2 42) 3

52

(.003 x 21) + (.0 (.088 88 x 22 )

43)  Atoms C: 1s22s22p4  Al: 1s22s22p63s23p1 S : 1s22s22p63s23p4  Ar: 1s22s22p63s23p6 Ca: 1s22s22p63s23p64s2 Se: 1s22s22p63s23p63d104S24p4 Ions Li+ : 1s2

Mg 2+ : 1s22s22p6 K + : 1s22s22p63s23p6 F- : 1s22s22p6 S2- : 1s22s22p63s23p6  As3- : 1s22s22p63s23p63d104s24p6

Answers to Questions 44) n = 1 : -2.178 x 10-18  J n = 2 : -5.45 x 10-19 J n = 3: -2.42 x 10-19 J 45) 7.32 x 1019 Hz 46) 4.73 x 1014 Hz 47) 3.75 x 10-7 meters 48) 4.99 x 10-7 meters 49) 5.64 x 10-19 Joules 50) 3.33 x 10-13 Joules 51) 3.10 x 10-19 Joules 52) 4.89 x 10-15 Joules 53) 2.78 meters

Copyright © 2014. E3 Scholastic Publishing.

SurvivingChem.com

Surviving Chemistry Books Student and teacher friendly supplemental instructional books and exam preps for high school chemistry and biology

WHICH OF OUR BOOKS IS RIGHT FOR YOUR STUDENTS?

Let them choose from our

eBook School-license Deals  As low as

$1  per book  Take an additional 10 - 40% off on SurvivingChem.com

Our eBook Platform  Online based; no downloading and no software to install.  Quick and and easy access for all of your students anytime, students anytime, anywhere.  Compatible with all brands of computers and browsers.  Mobile eBook format for on-the-go access with iPad, tablet or phone.  Visually stunning digital flipbook for students.  Easy to browse, read, search and print pages.  No screen advertisements to annoy and distract students.  Customized specifically for your school.

Easy to Order Visit SurvivingChem.com  

Choose a School-License Deal Select title(s) f rom rom our 7 books



Apply a discount code if applicable



Pay securely

For Ins Instant tant Preview