8.1 Periodic table Flashcards

1
Q

How is periodic table structured

A

List of elements in order of atomic number.

Metals on left, transition metals in centre, non metals on right.
Metalloids run diagonal, splitting metals and non metals

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2
Q

How are metals and non metals split

A

staircase line: divides them.

Metalloids touch this line, eg Silicon, which have a combination of metallic and non metallic properties

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3
Q

What did Mendeleev do

A

. Realised there were undiscovered elements, so left gaps for them .
. Arranged the known ones, so similar ones lined up in columns
. Since then new ones were discovered which fit the gaps, so he predicted the properties of missing elements

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4
Q

Lanthanides and actinides

A

The bottom block of the periodic table, they’re omitted

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5
Q

Where is the s block of periodic table, what is it

A

Far left, group 1 and 2
Elements that have their highest energy electrons in s orbitals are in the s block

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6
Q

Where is p block of periodic table
What is it

A

Far right, group 3,4,5,6,7,0
Elements that have their highest energy electrons in p orbitals are called p block

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7
Q

Where is d block
What is it

A

Centre, transition metals
Elements that have their highest energy electrons in the d orbitals are the d block

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8
Q

Where is F block
What is it

A

Under periodic table, the lanthanides and actinides.
Elements that have their highest energy electrons in f orbitals.

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9
Q

Why are transition metal elements and d block not the same

A

. Scandium and zinc aren’t transition metals because they don’t form any compounds that have partly filled d orbitals, which is the characteristic of transition metals.

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10
Q

Why are they called S, D, P,F blocks
How do you remember the order

A

When elements are heated they give out light energy at certain wavelengths, and as excited electrons fall back from one energy level to another.
This causes lines to appear on spectrum of light they give out.

Letters stand for words given to describe the light eg d for diffuse

Super duper power

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11
Q

What is a group

A

Vertical column of elements, elements in the same group have similar properties, and same number of electrons on outer shell.

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12
Q

How does reactivity in S block change down the group

A

Elements get more reactive going down group

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13
Q

How does Reactivity change down the P block

A

Elements get more reactive going up the group

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14
Q

Transition metal reactivity/ d block

A

They’re all quite unreactive, lots of useful metals are found here

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15
Q

Actinide properties

A

All radioactive eg uranium and thorium form naturally in earths crust

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16
Q

What are periods

A

. Horizontal rows of elements eg period 1 only has hydrogen and helium

17
Q

How are hydrogen and helium placed

A

. Helium above noble gases because of its properties, but it isn’t a p block element, its electron arrangement is 1s^2

. Hydrogen is above group 1, and forms 1+ ions (H+) like the group 1s. However hydrogen is a gas, and not a metal.