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Topic 2 SL

カード 66枚 作成者: Rink (作成日: 2016/06/14)

  • where are protons and neutrons located

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  • 1

    where are protons and neutrons located

    補足(例文と訳など)

    答え

    • in the nucleus of the atom

    解説

  • 2

    where are electrons located

    補足(例文と訳など)

    答え

    • in energy levels surrounding the nucleus

    解説

  • 3

    what is sub-atomic particle when relative charge = +1 and relative mass = 1

    補足(例文と訳など)

    答え

    • proton

    解説

  • 4

    what is sub-atomic particle when relative charge = no charge and relative mass = 1

    補足(例文と訳など)

    答え

    • neutron

    解説

  • 5

    what is sub-atomic particle when relative charge = -1 and relative mass = 1/2000

    補足(例文と訳など)

    答え

    • electron

    解説

  • 6

    each main energy level can be split into?

    補足(例文と訳など)

    答え

    • sub levels

    解説

  • 7

    the main energy level closest to the nucleus (n=1) has lowest or highest energy?

    補足(例文と訳など)

    答え

    • lowest energy

    解説

  • 8

    how many sub level does n=1 have?

    補足(例文と訳など)

    答え

    • sub level (1s)

    解説

  • 9

    n=2 has

    補足(例文と訳など)

    答え

    • 2sub levels (2s 2p)

    解説

  • 10

    n=3 of sub level

    補足(例文と訳など)

    答え

    • 3 sub levels (3s 3p 3d)

    解説

  • 11

    how many electrons in sub levels and number of electrons in main energy level when n=4 and 4 sub level (4s, 4p, 4d, 4f)

    補足(例文と訳など)

    答え

    • number of electrons in sub levels= 2, 6, 10, 14 number of electrons in main energy level= 32

    解説

  • 12

    nucleus symbol notation what is X?

    補足(例文と訳など)

    答え

    • symbol of element

    解説

  • 13

    nucleus symbol notation what is A?

    補足(例文と訳など)

    答え

    • mass number the number of protons plus the number of neutrons in the nucleus of an atom

    解説

  • 14

    nucleus symbol notation what is Z

    補足(例文と訳など)

    答え

    • atomic number the number of protons in the nucleus of an atom

    解説

  • 15

    A=12 Z=6 X=C what is proton, neutrons, electrons

    補足(例文と訳など)

    答え

    • proton= 6 neutron= 6 electron 6

    解説

  • 16

    calculate proton, neutron and electron

    補足(例文と訳など)

    答え

    • proton 20 neutron 20 electron 18

    解説

  • 17

    calculate proton, neutron and electron

    補足(例文と訳など)

    答え

    • protons 35 neutrons 46 electrons 36

    解説

  • 18

    what is isotopes?

    補足(例文と訳など)

    答え

    • atoms of the same element that have the same number of protons (same atomic number) but different numbers of neutrons (different mass number)

    解説

  • 19

    what is the name of the graph? y axis = percentage abundance (%) X axis = mass/ charge ratio

    補足(例文と訳など)

    答え

    • mass spectrum

    解説

  • 20

    how to calculate relative atomic mass

    補足(例文と訳など)

    答え

    • percentage abundance (%) × (mass/ charge ratio ) then divided by 100

    解説

  • 21

    europium (Ar= 151.96) has two naturally isotopes, ^151 EU and ^153 Eu. calculate the percentage abundance of each isotopes.

    補足(例文と訳など)

    答え

    • 153 and 151 are the mass numbers of the isotopes

    解説

  • 22

    europium (Ar= 151.96) has two naturally isotopes, ^151 EU and ^153 Eu. calculate the percentage abundance of each isotopes. part2

    補足(例文と訳など)

    答え

    • part 2

    解説

  • 23

    atomic orbitals represent?

    補足(例文と訳など)

    答え

    • a region of space where there is a high probability of finding an electron

    解説

  • 24

    according to Pauli exclusion principle

    補足(例文と訳など)

    答え

    • s orbitals are spherical. each s orbital can hold a maximum of 2 electrons with opposite spins

    解説

  • 25

    what is the shape of p orbital how many electrons can it hold?

    補足(例文と訳など)

    答え

    • dumbbell shape each o orbitals can hold a maximum of 2 electrons with opposite spins ( total of 6 electrons in the p sub level)

    解説

  • 26

    What is Aufbau principle used to determine?

    補足(例文と訳など)

    答え

    • The electron configuration of an atom or ion

    解説

  • 27

    Does the energy of orbitals increase or decrease?

    補足(例文と訳など)

    答え

    • Increase

    解説

  • 28

    What is the order in which the electrons fill the orbitals in an atom?

    補足(例文と訳など)

    答え

    • 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f

    解説

  • 29

    What is lowest energy orbital?

    補足(例文と訳など)

    答え

    • 1s

    解説

  • 30

    What is highest energy orbital?

    補足(例文と訳など)

    答え

    • 5f

    解説

  • 31

    Which energy orbital is higher? 3d > 4s or 3d < 4s

    補足(例文と訳など)

    答え

    • 3d > 4s

    解説

    so we fill 4s orbitals before 3d 1s 2s 2p 3s 3p 4s 3d manganese (Mn) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5

  • 32

    What is Pauli exclusion principle?

    補足(例文と訳など)

    答え

    • An atomic orbital can hold two electrons with opposite spins.

    解説

  • 33

    What does single headed arrow represent?

    補足(例文と訳など)

    答え

    • Electrons

    解説

  • 34

    What is Hund’s rule?

    補足(例文と訳など)

    答え

    • Degenerate orbitals in sub-level are singly occupied, and the electrons have the same spin.

    解説

    Used in 2p, 3p 4p 4d 4f 5p 5d 5f

  • 35

    What is the electron configuration of sodium (Na)

    補足(例文と訳など)

    答え

    • 1s2^ 2s^2 2p^6 3s^1

    解説

  • 36

    What is the electron configuration of manganese (Mn)?

    補足(例文と訳など)

    答え

    • 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5

    解説

  • 37

    How is electro configuration written

    補足(例文と訳など)

    答え

    • 1s^2

    解説

    1= main energy level s= sub level (s,p,d f) ^2 = number of electrons in sub-level

  • 38

    Write abbreviated electronic configurations for Na

    補足(例文と訳など)

    答え

    • Na [Ne] 3s^1

    解説

    Ne = 1s^2 2s^2 2p6 Ne is used from Na to Ar

  • 39

    Write abbreviated electronic configurations for K

    補足(例文と訳など)

    答え

    • [Ar] 4s^1

    解説

    Ar = 1s^2 2s^2 2p^6 3s^2 3p^6 Ar is used from K to Kr

  • 40

    What does electromagnetic spectrum show

    補足(例文と訳など)

    答え

    • all the frequencies of electromagnetic radiation

    解説

  • 41

    What is wave length?

    補足(例文と訳など)

    答え

    • distance between 2 crest

    解説

  • 42

    Higher frequency ................... Wavelength

    補足(例文と訳など)

    答え

    • Shorter

    解説

  • 43

    Low frequency ........... wavelength

    補足(例文と訳など)

    答え

    • Longer

    解説

  • 44

    Energy increases from

    補足(例文と訳など)

    答え

    • Radio, Microwaves, Infrared, Visible Light, Ultraviolet, X-rays, Gamma rays

    解説

    from right to left

  • 45

    high energy = ........ frequency =..........wavelength

    補足(例文と訳など)

    答え

    • high short

    解説

    high frequency = high frequency = short wavelength

  • 46

    Low energy =........ frequency = ....... wavelegth

    補足(例文と訳など)

    答え

    • Low Long

    解説

    low energy = low frequency = long wavelength

  • 47

    For visible light, which color is low frequency? red or blue

    補足(例文と訳など)

    答え

    • red

    解説

  • 48

    Continuos spectrum shows?

    補足(例文と訳など)

    答え

    • all wavelengths of visible light

    解説

  • 49

    Absorption line spectrum shows

    補足(例文と訳など)

    答え

    • black lines on colored background

    解説

    certain wavelength missing

  • 50

    Emission line spectrum shows

    補足(例文と訳など)

    答え

    • colored lines on a black background

    解説

    only certain wavelengths visible

  • 51

    Electrons can only exist at ...?

    補足(例文と訳など)

    答え

    • certain energy levels with discrete amounts of energy.

    解説

    it can be on n=1, n=2, etc but can't be in the middle of n=1 and n=2

  • 52

    Electrons can transition between ..... ?

    補足(例文と訳など)

    答え

    • energy levels

    解説

    electrons can transition from n=1 to n= 2. or n=3 to n=2

  • 53

    excited state is?

    補足(例文と訳など)

    答え

    • if an electron absorbs a discrete amount of energy, it can transition to a higher energy level

    解説

    If an electron emits a discrete amount of energy, it can transition to a lower energy level.

  • 54

    Reason for black lines on absorption spectrum is ?

    補足(例文と訳など)

    答え

    • the electron transition the between n=2 to n=3 electrons have absorb the energy and the energy that absorbs corresponds to the wavelength of visible light.

    解説

    n=2 to n=3 n=2 to n=4 n=2 to n=5 n=2 to n=6

  • 55

    Reasons for colored lines on black background of the emission spectrum is

    補足(例文と訳など)

    答え

    • corresponds to energy emitted and the electron transition higher energy level to lower energy level

    解説

  • 56

    what are electromagnetic radiations in Hydrogen emission spectrum?

    補足(例文と訳など)

    答え

    • UV-light Visible Light Infrared radiation

    解説

    UV-light n=1, ground state Visible Light n=2 Infrared radiation n=3

  • 57

    Transition to n=1 UV radiation has ...... energy, ..... frequency, ..... waveletgh

    補足(例文と訳など)

    答え

    • highest high short

    解説

  • 58

    Transition to n=2 visible light has violet = ...... energy red= ....... energy

    補足(例文と訳など)

    答え

    • highest lowest

    解説

    violet is highest energy red is lowest energy

  • 59

    Transitions to n=3 infrared radiation ..... energy ..... frequency ..... wavelength

    補足(例文と訳など)

    答え

    • lowest low longest

    解説

  • 60

    abbreviate electronic configurations use [......... gas]

    補足(例文と訳など)

    答え

    • noble

    解説

  • 61

    補足(例文と訳など)

    答え

    解説

  • 62

    Electronic configuration of ions focus on ..... block elements lose their ... electrons first when they form ions

    補足(例文と訳など)

    答え

    • d 4s

    解説

    Electronic configuration of ions focus on d block elements lose their 4s electrons first when they form ions

  • 63

    Write the electronic configuration for the Cu^2+ ion

    補足(例文と訳など)

    答え

    • Cu^2+ [Ar] 3d^9

    解説

    Cu 1s^2 2s^2 wp^6 3s^2 2p^6 4s^1 3d^10 Cu^2+ 1s^2 2s-2 2p^6 3s^2 3p^6 3d^9

  • 64

    orbital diagrams should be used to represent

    補足(例文と訳など)

    答え

    • the character and relative energy of orbitals

    解説

    Electronic configuration of Lithium 1s^2 2s^1

  • 65

    Hund's rule is

    補足(例文と訳など)

    答え

    • each degenerate orbital in a sub-level is singly occupied with one electron before being doubly occupied, and the electrons have the same spin.

    解説

    Nitrogen N 1s^2 2s^2 sp^3 Oxygen O 1s^2 2s^2 2p^4

  • 66

    draw orbital notation diagram of Fe^3+ ion

    補足(例文と訳など)

    答え

    • Fe~3+ 1s^2 2s^2 2p^6 3s^6 3d^5

    解説

    Fe atom 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6 Fe^3+ ion so -3 arrows lose 4s first then lose 3d Fe^3+ 1s^2 2s^2 2p^6 3s^2 3p^6 3d^5

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