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Trick or Treat

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#1 Which are the sublevels in an energy level of n = 2? a.s & f c.s, p, and d b.s & d d.s & p

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#1 D

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#2 Which of the following types of electromagnetic radiation has the highest frequency? a.X rays c.infrared light b. ultraviolet light d.microwaves

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#2 A

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#3 The fourth quantum number tells the… a.Energy level b.Spin state c.Orientation of orbital d.Orbital shape

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#3 B

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#4 The excited energy state of an atom is a.a higher state than its ground state b.its electron configuration. c.its principle quantum number. d.its ground state.

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#4 A

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#5 How many total electrons can a “d” sublevel hold? a.5 b.10 c.2 d.14

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#5 10

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#6 What are specific packets of energy called?

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#6 Quanta

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#7 What is the highest occupied energy level in an atom of Radon in its ground state? a. n = 4 b. n = 5 c. n = 6 d. n = 7

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#7 c. n = 6

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#8 How many electrons total can fit in the 3 energy level? a.18 b.10 c.9 d.8

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#8 a. 18

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#9 Number of wavelengths that pass by a point every second is described as……

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#9 Frequency

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#10 Which of the following statements is true? a. Each set of d orbitals can hold a maximum of 14 electrons. b. All s orbitals are spherically shaped. c. The first energy level contains only s and p orbitals. d. Each set of d orbitals contains seven orbitals.

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#10 B

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#11 Write the electron configuration of tin (Sn) (atomic # = 50):

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#11 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 2

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#12 The principle that states each electron occupies the lowest energy orbital available is the ______________. a. exclusion principle b. photoelectric principle c. uncertainty principle d. aufbau principle

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#12 D

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#13 How many electrons are in the highest energy p orbitals of a group IVA atom? a. 3 b. 1 c. 2 d. 4

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#13 C

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#14 The highest energy level in the ground state of Boron corresponds to the _________. a. zeroeth energy level b. second energy level c. first energy level d. third energy level

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#14 B

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#15 Which has the highest energy? Gamma rays Infrared rays Yellow light Microwaves Radio waves

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#15 Gamma Rays

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#16 Which one of the following electron configurations is incorrect? a. Cu-----[Ar]4s 1 3d 10 b. Ca-----1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 c. Xe-----[Kr] 5s 2 4d 10 5p 6 d. Mn-----[Ar]4s 2 4d 5

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#16 d. Mn-----[Ar]4s 2 4d 5

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#17 Draw the orbital notation of carbon:

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#17

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#18 How many orbitals are in n=3?

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#18 9

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#19 What is emitted when an electron moves from its excited state to its ground state?

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#19 A photon of light

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#20 Write the electron configuration of chromium (Cr) (atomic # = 24):

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#20 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 5

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#21 What are the four types of orbital shapes?

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#21 s, p, d, f

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#22 Write the noble gas notation of cesium (Cs):

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#22 [Xe] 6s 1

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#23 How many valence electrons does a group 1A metal atom have? a. 4 b. 2 c. 1 d. 3

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#23

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#24 Draw a periodic table and lable s, p, d, and f.

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#24

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#25 An element with the outermost electron configuration, ns 2 np 4, could be _______. a. Zr b. Se c. Pb d. Mo

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#25 b. Se

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#26 The total number of electrons in ALL s orbitals in a germanium atom is ________. a. 15 b. 6 c. 18 d. 8

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#26 d. 8

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#27 When an atom loses energy by electron transition, a(n) ___________ spectrum is produced. a. emission b. absorption c. ion d. adsorption

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#27 a. emission

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#28 The Heisenberg uncertainty principle states that ____________. a. no two electrons in the same atom can have the same set of four quantum numbers b. two atoms of the same element must have the same number of protons c. electrons of atoms in their ground states enter energetically equivalent sets of orbitals singly before they pair up in any orbital of the set d. it is impossible to simultaneously know the precise position and velocity of a particle

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#28 d. it is impossible to simultaneously know the precise position and velocity of a particle

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#29 An element whose atoms have four valence electrons is _______. a. Sn b. Nb c. Ti d. Cr

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#29 a. Sn

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#30 Name two elements that are exceptions to the Aufbau principle.

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#30 Copper and Chromium

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#31 What is the atomic # of the element with the noble-gas notation [Ne]3s 2 ?

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#31 Magnesium

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#32 As the wavelength of a wave increases, what happens to the frequency?

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#32 It decreases

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#33 What is the primary difference between a 2p x and a 3p x orbital?

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#33 Size

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#34 Describe Hund’s rule.

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#34 Empty bus seat rule

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#35 What is the primary difference between a 4p z and a 4p y orbital?

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#35 Orientation in space

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