Electron Structure Flashcards

1
Q

What is the electronic configuration of an atom?

A

describes the arrangement of electrons in shells

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2
Q

How are electrons placed?

A

Into shells starting with the lowest energy level first

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3
Q

how many electrons can the third and fourth shell hold?

A

-18
-32

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4
Q

What is an orbital?

A

A region around the nucleus that can hold two electrons, with opposite spins

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5
Q

What do the energy levels (shells) of principal quantum numbers contain instead of having precise energy values?

A

subshells

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6
Q

What do subshells contain?

A

-orbitals with different energy values

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7
Q

What spins can electrons have?

A

-up spins
-down spins

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8
Q

What is an electron?

A

-cloud of negative charge
-the negative charge cloud has the shape of the orbital occupied by the electron

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9
Q

what must two electrons in the same orbital have?

A

opposite spins

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10
Q

what are the different sub shells?

A

-S
-P
-D
-F

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11
Q

what is an s-subshell?

A

-contains one orbital (the s orbital)- it is an electron cloud with the shape of a sphere
-The greater the shell number (n), the greater the radius of it’s s-orbital

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12
Q

what is the p-sub shell?

A

contains 3-orbitals, each orbital is an electron cloud held within a dumb-bell shape

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13
Q

what is a d sub shell?

A

-Contains five orbitals

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14
Q

how many orbitals does an f-sub shell contain?

A

Seven orbitals

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15
Q

What happens to electrons in the same orbital?

A

They repel

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16
Q

What happens if we have orbitals with the same energy?

A

we put electrons in into individual orbitals before we pair them

17
Q

how do all electrons spin?

A

on axis: either clockwise or anti clockwise

18
Q

What is the electronic configuration for chromium and copper?

A

They both only contain one electron in the 4s (half filled)

19
Q

Why do chromium and copper have only one electron in the 4s orbital?

A

-by placing an electron into 3d sub shell, this creates either a full or half filled 3d orbital, which gives the atom increased stability

20
Q

when electrons are lost where are they lost from?

A

-Electron shells (when positive ions are formed)
-or will be added to the outer energy levels (when negative ions are formed)

21
Q

what happens when electrons are lost in transitional metal ions?

A

-The 4s are always lost before the 3d electrons (d-block elements)

22
Q

What is each block named after?

A

The subshell containing the highest energy electron for elements in that block