The Periodic Table and Periodicity Flashcards

1
Q

what groups in the periodic table are in the s-block

A

group 1 and 2

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2
Q

what groups in the periodic table are in the p-block

A

group 3 to 8

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3
Q

what groups in the periodic table are in the d-block

A

the transition metals (3 to 13 in a group 1 to 18 periodic table)

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4
Q

what is the general trend in the blocks as you go across them and why does the number of groups each block occupies make sense

A
  • there is one more electron in the outer shell for every group you go across (left to right)
  • this makes sense as the s orbital can only hold 2 electrons
  • so the s-block stops at group 1 and 2 which consist of an s orbital in their outer shells
  • the p-block consists of 6 groups
  • which matches with the 6 electrons a p subshell can hold with 3 p orbitals
  • the d subshell that has 5 d orbitals can hold 10 electrons
  • which matches with the ten ‘groups’ the d-block encompasses (the transition metals)
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5
Q

if the periodic table has the s-block on the left, d-block in the middle and p-block on the right, what does that imply about the actual order or arrangement of the periodic table

A
  • that the table is divided into blocks

- rather than simply groups and periods

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6
Q

what is the definition of peridicity

A
  • the regularly repeating pattern
  • of atomic, physical and chemical properties
  • with increasing atomic mass
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7
Q

what is the atomic radius of an element

A
  • the measure of the size of its atoms

- measured by the distance from the centre of the nucleus to the boundary of the electron cloud

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8
Q

since the atom doesnt have a well defined boundary, how is the atomic radius of an atom practically calculated

A
  • by determining the distance between two nuclei

- and dividing it by 2

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9
Q

what is the covelant radius of an atom

A

the radius of the atom when it is covelantly bonded with another atom

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10
Q

why are the covelant radii and atomic radii different, even for the same atom of the same element

A
  • when measuring the atomic radii practically, the boundaries of the two atoms would only be touching and not overlapping
  • this means that the distance between the two nuclei can be measured (diameter)
  • which would give you the radius of the atom
  • but for a covelantly bonded atom the boundaries of the electron clouds are overlapping
  • which means that the distance between the two nuclei (the diameter) would be decreased
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11
Q

why are the boundaries of the electron clouds overlapping for the covelantly bonded atoms whereas they are only touching for the other example

A
  • because covelant bonding consists of the sharing of electrons
  • so their outer shells would have to overlap to do this
  • whereas for the atomic example, there is no bond
  • so the outer shells dont interact with each other, they would more likely repel
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12
Q

which one between the covelant radius and atomic radius is usually shorter and why

A
  • the covelant radius
  • because the boundaries of their electrons clouds are overlapping
  • which means that the measured distance between the nuclei is smaller
  • leading to a smaller radius
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13
Q

what is the real name of the radius that can only be determined for group 8 elements (other than calling it the atomic radius)

A

the van der Waals radius

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14
Q

why can only one type of radius be determined for the group 8 elements

A
  • because they dont bond with other elements voluntarily

- so they can only have a ven der waals radius and not a covelant radius

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15
Q

what is the third radius called and what is it used for

A
  • the metallic radius

- which is used for metals

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16
Q

how does the atomic radii generally change across periods

A

the atomic radii decreases

17
Q

how does the nuclear charge change across the period and what is its effect

A
  • the nuclear charge increases due to the increase in protons in the nucleus
  • this leads to stronger electrostatic forces of attraction between the nucleus and the electrons which pulls them closer towards each other
  • causing the atomic radius to decrease
18
Q

how does the electron-electron repulsion change and what effect does this lead to

A
  • the number of electrons in the same quantum shell increases
  • which leads to an increased shielding effect that repels the electrons away from each other
  • causing the atomic radius to increase
19
Q

which changing factor proves to be more significant

A
  • the increase in the nuclear charge

- which causes the overall atomic radius to decrease across the periods

20
Q

the electronic configuration of Be is 1s2 2s2 whereas for B it is 1s2 2s2 2p1. knowing that these elements are in the first group and there should be a general increase in the first ionisation energies across a period, why is the first ionisation energy of B lower than that of Be if it has a larger nuclear charge

A
  • the boron atom has one electron in the 2p orbital meaning it is sitting at a higher energy level than the electrons in the 2s orbital
  • this means that less energy would be required in order to remove the electron
  • also, there is an increased effect of shielding experienced by the electron due to there being two inner subshells rather than just the one Be has
  • which leads to it having even more energy
  • which leads to a lower ionisaton energy being required
21
Q

N has an e.c. of 1s2, 2s2, 2p1, 2p1, 2p1
O hasan e.c. of 1s2, 2s2, 2p2, 2p1, 2p1
which element would have the lower first ionisation energy and why

A
  • the oxygen
  • because one of the electrons in the 2 p orbital that is full would be preferred to be removed first
  • the electron in this orbital experiences electron-electron repulsion from the other electron in its orbital
  • due to this the electron has a higher energy level
  • so the first ionisation energy would be less than nitrogen’s
22
Q

why would one of the electrons in the 2 p orbital that is full be preferred to be removed first

A
  • because the atom would simply prefer to have an equal share of electrons across the 3 p orbitals (2p1, 2p1, 2p1)
  • than having it as 2p2, 2p1, 2p0
  • as the pair of electrons in the p orbital already have higher energy levels
23
Q

if energy has to be supplied to the oxygen or boron atom in order for the electron to be removed, what does this imply about the energy levels of the ion

A

that the ion is energetically less stable than the atom