ap chemistry chapter 6 and 7 jeopardy

AP ChemistryAP ChemistryChapter 6 and 7 JeopardyChapter 6 and 7 Jeopardy

Jennie L. BordersJennie L. Borders

Round 1 – Chapter 6Round 1 – Chapter 6

VocabularyVocabulary WavesWaves EnergyEnergy De BroglieDe Broglie Quantum Quantum NumbersNumbers

Electron Electron Config.Config.

100 100 100 100 100 100

200 200 200 200 200 200

300 300 300 300 300 300

400 400 400 400 400 400

500 500 500 500 500 500

Round 2 – Chapter 7Round 2 – Chapter 7

Click to go to Round 2Click to go to Round 2

Vocabulary 100Vocabulary 100

What is Hund’s Rule?What is Hund’s Rule?

Hund’s Rule states that in Hund’s Rule states that in degenerate sublevels (p, d, and f) degenerate sublevels (p, d, and f)

the electrons are most stable when the electrons are most stable when they are unpaired.they are unpaired.


What is the Pauli Exclusion What is the Pauli Exclusion Principle?Principle?

The Pauli Exclusion Principle states The Pauli Exclusion Principle states that no two electrons will have the that no two electrons will have the

same quantum numbers, so when 2 same quantum numbers, so when 2 electrons occupy the same orbital, electrons occupy the same orbital,

then they must have opposite spins.then they must have opposite spins.


What is the Hiesenburg Uncertainty What is the Hiesenburg Uncertainty Principle and why is it irrelevant when Principle and why is it irrelevant when

referring to macroscopic objects?referring to macroscopic objects?

The Hiesenburg Uncertainty Principle states The Hiesenburg Uncertainty Principle states that it is impossible to know both the location that it is impossible to know both the location ad the speed (or momentum) of a particle. It ad the speed (or momentum) of a particle. It

does not apply to macroscopic objects does not apply to macroscopic objects because it is based on the formula because it is based on the formula = h/mv, = h/mv, and macroscopic objects have such a large and macroscopic objects have such a large mass that the uncertainly is extremely small.mass that the uncertainly is extremely small.

Vocabulary 400Vocabulary 400Why is the emission spectrum for Why is the emission spectrum for

hydrogen a line spectrum, and if hydrogen a line spectrum, and if hydrogen only has 1 electron, then hydrogen only has 1 electron, then how can more than one line exist?how can more than one line exist?

The hydrogen spectrum is not continuous The hydrogen spectrum is not continuous because energy is quantized, so electrons can because energy is quantized, so electrons can

inhabit only certain energy levels. There is inhabit only certain energy levels. There is more than one line because electrons of more than one line because electrons of different hydrogen atoms are jumping to different hydrogen atoms are jumping to

different levels.different levels.


What is blackbody radiation, the What is blackbody radiation, the photoelectric effect, and emission photoelectric effect, and emission

spectrum?spectrum?-Blackbody radiation is the phenomena that occurs -Blackbody radiation is the phenomena that occurs

when a heated object (metal) glows.when a heated object (metal) glows.-The photoelectric effect is when light of sufficient -The photoelectric effect is when light of sufficient energy shines on a metal surface and electrons energy shines on a metal surface and electrons

are ejected.are ejected.-An emission spectrum is when a substance (gas) -An emission spectrum is when a substance (gas) is heated until certain wavelengths of light is heated until certain wavelengths of light

are emitted from the movement of electrons.are emitted from the movement of electrons.

Waves 100Waves 100

Electromagnetic radiation travels Electromagnetic radiation travels through a vacuum at what speed?through a vacuum at what speed?

3.0 x 103.0 x 1088 m/s m/s

Waves 200Waves 200

What is the wavelength of light in What is the wavelength of light in meters that has a frequency of meters that has a frequency of

1.20 x 101.20 x 101313 s s-1-1??

c = c = v so v so = c/v = c/v

= = 3.0 x 103.0 x 1088 m/s m/s = = 2.5 x 102.5 x 10-5-5 m m 1.20 x 101.20 x 101313 /s /s

Waves 300Waves 300

What is the frequency of What is the frequency of electromagnetic radiation that has electromagnetic radiation that has a wavelength of 0.53 angstroms?a wavelength of 0.53 angstroms?

0.53 A x 0.53 A x 1m 1m = 5.3 x 10 = 5.3 x 10-11-11mm 1 x 101 x 101010AA

c = c = v so v = c/v so v = c/v = v = 3.0 x 103.0 x 1088 m/s m/s = = 5.66 x 105.66 x 101818 Hz Hz 5.3 x 105.3 x 10-11-11m m

Waves 400Waves 400

What is the wavelength of light in What is the wavelength of light in nm that has a frequency of nm that has a frequency of

4.62 x 104.62 x 101414 s s-1-1??

c = c = v so v so = c/v = c/v = = 3.0 x 103.0 x 1088m/sm/s = 6.49 x 10 = 6.49 x 10-7-7mm 4.62 x 104.62 x 101414 /s /s6.49 x 106.49 x 10-7-7m x m x 1 x 101 x 1099nmnm = = 649nm649nm 1m1m

Waves 500Waves 500

Of the following, _________ has the Of the following, _________ has the shortest wavelength.shortest wavelength.

a.a. X-rayX-ray

b.b. RadioRadio

c.c. MicrowaveMicrowave

d.d. UltravioletUltraviolet

e.e. Infrared Infrared

a. X-raya. X-ray

Energy 100Energy 100

The frequency of a photon that has The frequency of a photon that has an energy of 3.7 x 10an energy of 3.7 x 10-18-18J is what?J is what?

E = hv so v = E/hE = hv so v = E/hv = v = 3.7 x 10 3.7 x 10-18-18J J = = 5.58 x 105.58 x 101515 Hz Hz 6.62 x 106.62 x 10-34-34 J J..ss


What is the wavelength of a photon What is the wavelength of a photon that has an energy of 5.25 x 10that has an energy of 5.25 x 10-19-19J?J?

E = hv so v = E/hE = hv so v = E/hv = v = 5.25 x 10 5.25 x 10-19-19J J = 7.92 x 10= 7.92 x 101414 Hz Hz 6.62 x 106.62 x 10-34-34 J J..ss

c = c = v so v so = c/v = c/v = = 3.0 x 103.0 x 1088 m/s m/s = = 3.79 x 103.79 x 10-7-7 m m 7.92 x 107.92 x 101414 /s /s


What is the energy of a photon that What is the energy of a photon that has a wavelength of 9.0m?has a wavelength of 9.0m?

c = c = v so v = c/v so v = c/v = v = 3.0 x 103.0 x 1088 m/s m/s = 3.33 x 10 = 3.33 x 1077 /s /s 9.0 m9.0 m

E = hvE = hvE = 6.626 x 10E = 6.626 x 10-34-34 J J..s x 3.33 x 10s x 3.33 x 1077 /s = /s =

2.21 x 102.21 x 10-26-26 J J

Energy 400Energy 400What is the energy of a photon that What is the energy of a photon that

has a wavelength of 12.3 nm?has a wavelength of 12.3 nm?12.3 nm x 12.3 nm x 1m 1m = 1.23 x 10= 1.23 x 10-8-8mm 1 x 101 x 1099 nm nm

c = c = v so v = c/v so v = c/v = v = 3.0 x 103.0 x 1088 m/s m/s = 2.44 x 10 = 2.44 x 101616 /s /s 1.23 x 101.23 x 10-8-8 m m

E = hvE = hvE = 6.626 x 10E = 6.626 x 10-34-34 J J..s x 2.44 x 10s x 2.44 x 101616 /s = /s =

1.62 x 101.62 x 10-17-17 J J

Energy 500Energy 500A mole of yellow photons of wavelength A mole of yellow photons of wavelength

527 nm has how many kJ of energy?527 nm has how many kJ of energy?527 nm x 527 nm x 1m 1m = 5.27 x 10= 5.27 x 10-7-7mm 1 x 101 x 1099 nm nm

c = c = v so v = c/v so v = c/v = v = 3.0 x 103.0 x 1088 m/s m/s = 5.69 x 10 = 5.69 x 101414 /s /s 5.27 x 105.27 x 10-7-7 m m

E = hvE = hvE = 6.626 x 10E = 6.626 x 10-34-34 J J..s x 5.69 x 10s x 5.69 x 101414 /s = 3.77 x 10 /s = 3.77 x 10-19-19 J J3.77 x 103.77 x 10-19-19J x 6.02 x 10J x 6.02 x 102323 photons = 2.27 x 10 photons = 2.27 x 1055JJ2.27 x 102.27 x 1055 J x J x 1kJ 1kJ = = 227kJ227kJ 1000 J1000 J

De Broglie 100De Broglie 100

What is the wavelength in meters of a What is the wavelength in meters of a 2.0 kg object moving at a speed of 50 2.0 kg object moving at a speed of 50

m/s?m/s?

= h/mv= h/mv= = 6.626 x 106.626 x 10-34-34 J J..ss = = 6.63 x 106.63 x 10-36-36mm 2.0kg x 50m/s2.0kg x 50m/s


What is the wavelength in meters of a What is the wavelength in meters of a 25g object moving at a speed of 5.0 25g object moving at a speed of 5.0

m/s?m/s?

25g x 25g x 1kg 1kg = 0.025kg = 0.025kg 1000g1000g

= h/mv= h/mv= = 6.626 x 106.626 x 10-34-34 J J..ss = = 5.30 x 105.30 x 10-33-33mm 0.025kg x 5.0m/s0.025kg x 5.0m/s


The wavelength of an electron is 8.7 x The wavelength of an electron is 8.7 x 1010-11-11m. The mass of the electron is m. The mass of the electron is 9.1 x 109.1 x 10-31-31kg. What is the velocity in kg. What is the velocity in

m/s?m/s? = h/mv so v = h/= h/mv so v = h/mm

= = 6.626 x 10 6.626 x 10-34-34 J J..s s = = 8.7 x 108.7 x 10-11-11m x 9.1 x 10m x 9.1 x 10-31-31kgkg

8.37 x 108.37 x 1066m/sm/s

De Broglie 400De Broglie 400At what speed in m/s must a 10.0mg At what speed in m/s must a 10.0mg

object be moving to have a object be moving to have a wavelength of 3.3 x 10wavelength of 3.3 x 10-41-41m?m?

10mg x 10mg x 1g 1g x x 1kg 1kg = 1 x 10 = 1 x 10-5-5kgkg 1000mg 1000g1000mg 1000g

= h/mv so v = h/= h/mv so v = h/mmv = v = 6.626 x 10 6.626 x 10-34-34 J J..s s = = 3.3 x 103.3 x 10-41-41m x 1 x 10m x 1 x 10-5-5kgkg

2.01 x 102.01 x 1012 12 m/sm/s

De Broglie 500De Broglie 500What is the wavelength of a car with a What is the wavelength of a car with a

mass of 1.0 x 10mass of 1.0 x 1033kg traveling at 75 kg traveling at 75 km/hr?km/hr?

75 75 kmkm x x 1hr 1hr x x 1000m1000m = 20.83 m/s = 20.83 m/s hr 3600s 1kmhr 3600s 1km

= h/mv= h/mv= = 6.626 x 10 6.626 x 10-34-34 J J..s s = = 1 x 101 x 1033kg x 20.83m/skg x 20.83m/s

3.18 x 103.18 x 10-38-38mm

Quantum Numbers 100Quantum Numbers 100

Which of the following sets of Which of the following sets of quantum numbers is not possible?quantum numbers is not possible?

a.a. 2, 0, 02, 0, 0b.b. 2, 1, -12, 1, -1c.c. 3, 1, -13, 1, -1d.d. 1, 1, 11, 1, 1e.e. 3, 2, 13, 2, 1d. 1, 1, 1d. 1, 1, 1


Which of the following is an appropriate Which of the following is an appropriate set of quantum numbers?set of quantum numbers?

a.a. 2, 2, -1, -½ 2, 2, -1, -½

b.b. 1, 0, 0, ½ 1, 0, 0, ½

c.c. 3, 3, 3, ½ 3, 3, 3, ½

d.d. 5, 4, -5, ½ 5, 4, -5, ½

e.e. 3, 3, 3, -½ 3, 3, 3, -½

b. 1, 0, 0, ½ b. 1, 0, 0, ½


What are the correct quantum What are the correct quantum numbers for the highest electron in numbers for the highest electron in

bromine?bromine?

Br (35eBr (35e--))[Ar] 3d[Ar] 3d10104s4s224p4p5 5 __ __ ____ __ __ 4p4p

4, 1, 1, ½4, 1, 1, ½Other accepted answers would be quantum Other accepted answers would be quantum

numbers for any of the 4p electrons.numbers for any of the 4p electrons.

↑↓↑↓ ↑↓↑↓ ↑↑

Quantum Numbers 400Quantum Numbers 400What are the quantum numbers for What are the quantum numbers for

the last electron in gold when it is the last electron in gold when it is not rearranged?not rearranged?

Au (79 eAu (79 e--))__ __ __ __ ____ __ __ __ __

5d5d5, 2, 2, ½5, 2, 2, ½

Other accepted answers would be quantum numbers for any of Other accepted answers would be quantum numbers for any of the 5d electrons.the 5d electrons.

↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓↑↓ ↑↑


What are the quantum numbers for What are the quantum numbers for the highest electron in a nitrogen the highest electron in a nitrogen

ion?ion?

NN3-3- (10 e (10 e--))__ __ ____ __ __

2p2p2, 1, 1, -½ 2, 1, 1, -½

Other accepted answers would be quantum numbers for any of the Other accepted answers would be quantum numbers for any of the 2p electrons.2p electrons.

↑↓↑↓ ↑↓↑↓ ↑↑↓↓

Electron Configuration 100Electron Configuration 100

What is the noble gas configuration What is the noble gas configuration for a ground state silver atom?for a ground state silver atom?

Ag (47 eAg (47 e--))[Kr]4d[Kr]4d995s5s22


Which one of the following Which one of the following configurations depicts an excited configurations depicts an excited

oxygen atom?oxygen atom?a.a. 1s1s222s2s222p2p22

b.b. 1s1s222s2s222p2p223s3s22

c.c. 1s1s222s2s222p2p11

d.d. 1s1s222s2s222p2p44

e.e. [He]2s[He]2s222p2p44

b. 1sb. 1s222s2s222p2p223s3s22


What element has a valence What element has a valence configuration of 4sconfiguration of 4s11??

KK


The valence shell of the element X The valence shell of the element X contains 2 electrons in a 5s contains 2 electrons in a 5s

subshell. Below that shell, element subshell. Below that shell, element X has a partially filled 4d subshell. X has a partially filled 4d subshell.

What type of element is X?What type of element is X?

transition metaltransition metal


What is the condensed configuration What is the condensed configuration for Polonium?for Polonium?

Po (84 ePo (84 e--))1s1s222s2s222p2p663s3s223p3p663d3d10104s4s224p4p664d4d101044

ff14145s5s225p5p665d5d10106s6s226p6p44

ZZeffeff RadiusRadius Ionization Ionization EnergyEnergy

Electro-Electro-negativitynegativity

Electron Electron AffinityAffinity

Metals vs. Metals vs. NonmetalsNonmetals

200 200 200 200 200 200

400 400 400 400 400 400

600 600 600 600 600 600

800 800 800 800 800 800

1000 1000 1000 1000 1000 1000

ZZeffeff 200 200

What is the effective nuclear charge?What is the effective nuclear charge?

The attraction of the positively The attraction of the positively charged nucleus for a negatively charged nucleus for a negatively charged electron that takes into charged electron that takes into account the shielding effect of account the shielding effect of

the core electrons.the core electrons.

ZZeffeff 400 400

Which of the following has the greater Which of the following has the greater effective nuclear charge, calcium effective nuclear charge, calcium

or chlorine?or chlorine?

ClCl

ZZeffeff 600 600

What is the formula for calculating What is the formula for calculating effective nuclear charge and what effective nuclear charge and what

do the variables mean?do the variables mean?

ZZeffeff = Z – S = Z – S

Z = nuclear chargeZ = nuclear chargeS = shielding (core electrons)S = shielding (core electrons)

ZZeffeff 800 800

Explain the trend for effective nuclear Explain the trend for effective nuclear charge going across a period.charge going across a period.

ZZeffeff increases as you move increases as you move

across a period because across a period because electrons are being added to the electrons are being added to the same energy level so there is not same energy level so there is not added shielding, but protons are added shielding, but protons are being added to the nucleus, so being added to the nucleus, so

the nuclear charge is increasing.the nuclear charge is increasing.

ZZeffeff 1000 1000Explain the trend for effective nuclear Explain the trend for effective nuclear

charge going down a group.charge going down a group.

ZZeffeff increases slightly as you move increases slightly as you move

down a group because the nuclear down a group because the nuclear charge greatly increases as we move charge greatly increases as we move

down a group and as electrons are down a group and as electrons are added to higher and higher energy added to higher and higher energy

levels that are farther from the nucleus, levels that are farther from the nucleus, they are less capable of shielding the they are less capable of shielding the

valence electrons.valence electrons.

Radius 200Radius 200

Explain the trend for atomic radius as Explain the trend for atomic radius as you move down a group.you move down a group.

Atomic radius increases as you Atomic radius increases as you move down a group because move down a group because electrons are added to higher electrons are added to higher energy levels that are further energy levels that are further

away from the nucleus.away from the nucleus.

Radius 400Radius 400Explain the trend for atomic radius as Explain the trend for atomic radius as

you move across a period.you move across a period.Atomic radius decreases as you move Atomic radius decreases as you move across a period because electrons are across a period because electrons are being added to the same energy level being added to the same energy level and Zand Zeffeff increases meaning that more increases meaning that more

protons are being added. The larger protons are being added. The larger nuclear charge allows the nucleus a nuclear charge allows the nucleus a

greater attraction to pull the electrons greater attraction to pull the electrons closer.closer.


Put the following in order of Put the following in order of increasing radius: Kincreasing radius: K++, Cl, Cl--, Ca, Ca2+2+, and , and

SS2-2-..

CaCa2+2+, K, K++, Cl, Cl--, S, S2-2-


Explain the trend for ionic radius as Explain the trend for ionic radius as you move down a group.you move down a group.

Ionic radius increases as you Ionic radius increases as you move down a group because move down a group because each time you move down, a each time you move down, a

new larger energy level is added new larger energy level is added that is farther from the nucleus.that is farther from the nucleus.

Radius 1000Radius 1000Explain the trend for ionic radius as Explain the trend for ionic radius as

you move across a period.you move across a period.Cations are on the left side of the periodic table and Cations are on the left side of the periodic table and lose valence electrons. Anions are on the right side lose valence electrons. Anions are on the right side

of the periodic table and gain electrons. When of the periodic table and gain electrons. When moving from left to right in the cations, elements lose moving from left to right in the cations, elements lose

one more electron than the previous element but one more electron than the previous element but also gain one proton. Since cations lose electrons also gain one proton. Since cations lose electrons

they are smaller than their parent atom and the they are smaller than their parent atom and the protons pull the remaining electrons in. As more protons pull the remaining electrons in. As more electrons are lost when moving left to right the electrons are lost when moving left to right the

increases nuclear charge causes the ionic radius to increases nuclear charge causes the ionic radius to decrease. decrease.

Radius 1000 (con’t)Radius 1000 (con’t)Explain the trend for ionic radius as you move Explain the trend for ionic radius as you move

across a period.across a period.Anions are larger than their parent atoms due to Anions are larger than their parent atoms due to

electron-electron repulsions from added electrons. electron-electron repulsions from added electrons. Between cations and anions, there is an increase in Between cations and anions, there is an increase in

ionic size. When moving from left to right in the ionic size. When moving from left to right in the anions, elements gain one less electron than the anions, elements gain one less electron than the previous element. Since the electrons are being previous element. Since the electrons are being

added to the same energy level but no protons are added to the same energy level but no protons are being added, electron-electron repulsions cause the being added, electron-electron repulsions cause the

electrons to spread out. As fewer electrons are electrons to spread out. As fewer electrons are added, this repulsion is smaller resulting in a added, this repulsion is smaller resulting in a

decreases from left to right for anions. Overall, ionic decreases from left to right for anions. Overall, ionic radius decreases as you move across a period.radius decreases as you move across a period.

Ionization Energy 200Ionization Energy 200

What is ionization energy?What is ionization energy?

Ionization energy is the energy Ionization energy is the energy needed to remove one electron needed to remove one electron

from a gaseous atom.from a gaseous atom.


Which element has the higher Which element has the higher ionization energy, fluorine or ionization energy, fluorine or

bromine?bromine?

FluorineFluorine


An element is on the third row of the An element is on the third row of the periodic table and has the periodic table and has the

following ionization energies, what following ionization energies, what is the element?is the element?

II11 = 578 I = 578 I22 = 1817 I = 1817 I33 = 2745 I = 2745 I44 = 11,577 = 11,577

AlAl


Explain the trend of ionization energy Explain the trend of ionization energy going down a group.going down a group.

Ionization energy is the energy needed to remove Ionization energy is the energy needed to remove an electron from a gaseous atom. Ionization an electron from a gaseous atom. Ionization

energy decreases as you move down a group energy decreases as you move down a group because you add larger energy levels which are because you add larger energy levels which are farther from the nucleus. There is also increases farther from the nucleus. There is also increases

shielding from a larger core of electrons. As a shielding from a larger core of electrons. As a valence electron is farther from the nucleus and valence electron is farther from the nucleus and

shielded by more electrons, it takes less energy to shielded by more electrons, it takes less energy to

remove it because the nucleus has less of a pull.remove it because the nucleus has less of a pull.


Explain the trend for ionization energy as Explain the trend for ionization energy as you move across a period.you move across a period.

Ionization energy is the energy needed to Ionization energy is the energy needed to remove one electron from a gaseous atom. As remove one electron from a gaseous atom. As you move across a period, electrons are added you move across a period, electrons are added to the same energy level and protons are added to the same energy level and protons are added to the nucleus. Since electrons are added to the to the nucleus. Since electrons are added to the

same energy level, there is no increases same energy level, there is no increases shielding. Since protons are added to the shielding. Since protons are added to the

nucleus, the effective nuclear charge increases, nucleus, the effective nuclear charge increases, so it takes more energy to remove an electron.so it takes more energy to remove an electron.

Electronegativity 200Electronegativity 200

What is electronegativity?What is electronegativity?

Electronegativity is the attraction Electronegativity is the attraction of an atom in a compound for an of an atom in a compound for an

electron.electron.


Which element is more Which element is more electronegative, silicon or electronegative, silicon or

chlorine?chlorine?

ClCl


Which element is more Which element is more electronegative, nitrogen or electronegative, nitrogen or

gallium?gallium?

NN


Explain the trend for electronegativity Explain the trend for electronegativity as you move down a group.as you move down a group.

Electronegativity is the attraction of an atom in Electronegativity is the attraction of an atom in a compound for an electron. As you move a compound for an electron. As you move

down a group, electrons are added to larger down a group, electrons are added to larger energy levels that are more shielded and energy levels that are more shielded and

farther from the nucleus. Since the electrons farther from the nucleus. Since the electrons shared or transferred in a compound are shared or transferred in a compound are

valence shell (outer energy level) electrons, valence shell (outer energy level) electrons, the nucleus down not have much attraction the nucleus down not have much attraction

due to increased shielding and distance.due to increased shielding and distance.

Electronegativity 1000Electronegativity 1000Explain the trend for electronegativity Explain the trend for electronegativity

as you move across a period.as you move across a period.Electronegativity is the attraction of an atom in a Electronegativity is the attraction of an atom in a compound for an electron. As you move across a compound for an electron. As you move across a period, electrons are added to the same energy period, electrons are added to the same energy

level, so there is no increased shielding, but level, so there is no increased shielding, but protons are added to the nucleus. Since there is protons are added to the nucleus. Since there is

an increase in nuclear charge with constant an increase in nuclear charge with constant shielding, Zshielding, Zeffeff increases. Since effective nuclear increases. Since effective nuclear

charge increases, the nucleus has more attraction charge increases, the nucleus has more attraction fro the valence electrons, so the is more attraction fro the valence electrons, so the is more attraction

for the valence electrons from another atom in for the valence electrons from another atom in order to gain a full octet.order to gain a full octet.

Electron Affinity 200Electron Affinity 200

What is the definition of electron What is the definition of electron affinity?affinity?

Electron affinity is the attraction Electron affinity is the attraction of a gaseous atom for one extra of a gaseous atom for one extra

electron.electron.


Which element has the lower electron Which element has the lower electron affinity, iodine or tin?affinity, iodine or tin?

SnSn


Which element has the higher Which element has the higher electron affinity, sulfur or lead?electron affinity, sulfur or lead?

SS

Electron Affinity 800Electron Affinity 800Explain the trend for electron affinity Explain the trend for electron affinity

going across a period.going across a period.Electron affinity is the attraction of a gaseous atom Electron affinity is the attraction of a gaseous atom

for one extra electron. As you move across a for one extra electron. As you move across a period, electrons are added to the same energy period, electrons are added to the same energy level so shielding does not change. Protons are level so shielding does not change. Protons are

also added so the nuclear charge increases. Since also added so the nuclear charge increases. Since nuclear charge increases and shielding remain nuclear charge increases and shielding remain constant, effective nuclear charge increases, so constant, effective nuclear charge increases, so

the attraction of the nucleus for the electrons the attraction of the nucleus for the electrons increases. Electron affinity increases as you move increases. Electron affinity increases as you move

across a period.across a period.

Electron Affinity 1000Electron Affinity 1000Explain the trend for electron affinity Explain the trend for electron affinity

going down a group.going down a group.

Electron affinity is the attraction of a gaseous atom Electron affinity is the attraction of a gaseous atom for one extra electron. As you go down a group, for one extra electron. As you go down a group, electrons are added to larger energy levels that electrons are added to larger energy levels that are farther from the nucleus. This increases the are farther from the nucleus. This increases the

shielding because it increases the amount of core shielding because it increases the amount of core electrons. Since the valence electrons are at a electrons. Since the valence electrons are at a

further distance from the nucleus with increased further distance from the nucleus with increased shielding, the nucleus has a lower attraction for shielding, the nucleus has a lower attraction for

the added electrons. Electron affinity decreases as the added electrons. Electron affinity decreases as you move down a group.you move down a group.

Metals vs. Nonmetals 200Metals vs. Nonmetals 200

Can noble gases from compounds? If Can noble gases from compounds? If so, which one(s)?so, which one(s)?

Yes, Xe and recently Ar.Yes, Xe and recently Ar.


What are the colors of the first four What are the colors of the first four halogens?halogens?

F = pale yellowF = pale yellowCl = yellow-greenCl = yellow-green

Br = reddish-brownBr = reddish-brownI = dark gray (purple vapors)I = dark gray (purple vapors)


Compare two physical characteristics Compare two physical characteristics of alkali metals and alkaline earth of alkali metals and alkaline earth

metals.metals.

Alkali metals are soft and have Alkali metals are soft and have low melting points. Alkaline earth low melting points. Alkaline earth metals are hard and have higher metals are hard and have higher

melting points.melting points.


Explain how hydrogen can exist in 2 Explain how hydrogen can exist in 2 groups.groups.

Hydrogen belongs in the alkali metals Hydrogen belongs in the alkali metals group (group 1) because it tends to group (group 1) because it tends to form a +1 charge and has 1 valence form a +1 charge and has 1 valence electron, but it can also belong in the electron, but it can also belong in the halogens group (group 17) because it halogens group (group 17) because it

can form a -1 charge and it only can form a -1 charge and it only needs one more valence electron to needs one more valence electron to

have a complete octet.have a complete octet.


List 5 characteristics of metals and List 5 characteristics of metals and nonmetals.nonmetals.

MetalsMetalsSolids (except Hg)Solids (except Hg)

DuctileDuctileMalleableMalleable

Good conductorsGood conductorsCationsCations

Oxides are basicOxides are basicOxidized easilyOxidized easily

NonmetalsNonmetalsMost are gasesMost are gases

BrittleBrittlePoor conductorsPoor conductors

AnionsAnionsOxides are acidicOxides are acidicReduced easilyReduced easily

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