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chemisty > atomic struc > Flashcards

atomic struc Flashcards

1
Q

Atoms are made up of _____, _____, and _____.

A

protons, neutrons, electrons

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2
Q

protons and neutrons are found in

A

nucleus of atom

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3
Q

Electrons are located in

A

orbitals

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4
Q

relative mass of a proton

A

1

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5
Q

relative mass of neutron

A

1

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6
Q

Relative mass of an electron

A

1/1840

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7
Q

relative charge of proton

A

+1

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8
Q

relative charge of neutron

A

0 (neutral)

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9
Q

relative charge of electron

A

-1

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10
Q

deflection of proton in electric field

A

towards neg electrode

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11
Q

deflection of neutron in electric field

A

not deflected

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12
Q

deflection of electron in electric field

A

towards pos electrode

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13
Q

angle of deflection formula

A

charge/mass

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14
Q

this is a gd solution

A

angle of deflection = k(charge/mass), where k is proportionality constant

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15
Q

express angle of deflection to ___ dp

A

1

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16
Q

when drawing paths of deflection, deflections only starts from

A

start of electric field

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17
Q

atomic no. is

A

no. of protons

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18
Q

mass no. is

A

total no. of proton + neutron

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19
Q

nucleon no. is

A

no. of protons and neutrons

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20
Q

isotopes are ________ of the ________ _______________ which contain the ___________ number of ____________ but _________ no. of __________

A

atoms, same element, same, protons, diff, neutrons

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21
Q

isotopes of the same element have __________ chemical properties but ______________ physical properties

A

similar, different

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22
Q

isotopes are

A

atoms of the same element which contain the same no. of protons but diff. no. of neutrons

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23
Q

electrons in atom occupy specific region of space arnd nucleus known as an

A

orbital

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24
Q

arrangement of electrons in orbitals is called

A

electronic structure

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25
Q

each principal quantum shell (electronic shell) is assigned a

A

principal quantum no. n

26
Q

smaller value of n, _________ ___________ the electron bound to nucleus (bc electron________________ to proton)

A

more strongly, attracted

27
Q

smaller value of n, ________ the energy level of electron

A

lower

28
Q

eg: principal quantum shell n=1 is _______ __________ attracted to nucleus & has the ________ energy

A

most strongly, least

29
Q

each principal quantum shell is made up of 1/more subshells, that can be labelled as __,__,___ or ___

A

s p d f

30
Q

subshell is a ___________________with the _______ energy but _______ orientation in space

A

grp of orbitals, same, diff

31
Q

subshell s has ___________________

A

1 orbital (s orbital)

32
Q

subshell p has __________________

A

3 orbitals (px, py, pz)

33
Q

order of energy levels for subshells is___<____<____<____

A

s, p, d, f

34
Q

atomic orbitals def: a __________ of ________round the nucleus where there’s 95% probability of ______________________

A

region, space, locating the electron

35
Q

atomic orbitals def:

A

a region of space round the nucleus where there’s 95% probability of locating the electron

36
Q

each orbital can hold max ___ electrons

A

2

37
Q

s orbitals are ____________ in shape & _______________________

A

spherical, non-directional

38
Q

size of 1s orbital___ 2s orbital___3s orbital

A

<, <

39
Q

p orbitals has __ types, have _______________ shape & are ______________

A

3, dumb-bell, directional

40
Q

size of 2p orbital___3p orbital

A

<

41
Q

nearer orbital to nucleus, __________ its energy

A

lower

42
Q

in same principal quantum no., distance of orbital from nucleus is __>___>___, so energy of ___>____>___

A

d, p, s

43
Q

energy level of 2px___2py___2pz

A

=

44
Q

in energy level diagram, energy gap between 1s & 2s is __________ than energy gap between 2s & 3s

A

greater

45
Q

in energy level diagram, energy level of 4s is ________ than 3d orbital when they are empty

A

lower

46
Q

electronic configuration refers to

A

arrangement of electrons of its atoms in their shells, subshells & orbitals

47
Q

aufbau principle: electrons occupy _________ energy orbital ________ b4 occupying the ___________ energy orbitals. order of filling in orbitals: _______________________________________________________

A

lowest, first, higher, 1s 2s 2p 3s 3p 4s 3d 4p

48
Q

Pauli’s exclusion principle: each orbital can hold max _____ electrons & the ____ electrons have to be in _____________ spins (https://chemistrytalk.org/pauli-exclusion-principle)

A

2, 2, opposite

49
Q

Hund’s Rule: orbitals must be occupied ____________ b4 ____________ occurs to ensure electrons are as ______ apart as possible to ________________ electronic repulsion

A

singly, pairing, far, minimise

50
Q

if all rules r followed, resultant arrangement of electrons known as

A

ground state electronic configuration (lowest energy state)

51
Q

when 1/more electrons absorb energy & r promoted to higher energy level, atom is to be in an

A

excited state

52
Q

Isoelectronic def: atoms/ions with __________ electronic config.(same no. of electrons)

A

same

53
Q

Isoelectronic def: _____/______ with _______________________________________

A

atoms/ions, same electronic configuration

54
Q

Grp: _____________ columns of elements in periodic table

A

vertical

55
Q

elements in same grp have the ___________ no. of valence electrons–> ________ electronic config.–> _________ chem properties

A

same, same, similar

56
Q

elements of same grp have _______no. of principal quantum shells

A

diff

57
Q

period is ________________ rows of elements

A

horizontal

58
Q

period no.___no. of principal quantum shells

A

=

59
Q

elements in same period have ________________ of principal quantum shells

A

same no.

60
Q

elements of same period have _________ no. of valence electrons

A

diff

chemisty (6 decks)

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