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Honors chemistry > Chapter 4- The Periodic Table > Flashcards

Chapter 4- The Periodic Table Flashcards

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0
Q

Who is known as the father of the modern periodic table

A

Mendeleev

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1
Q

Mendeleev

A

Published 1st period table in 1869

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2
Q

How did Mendeleev arrange elements

A

In order of increasing atomic mass and by properties, both physical and Chemical

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3
Q

Moseley

A

Reorders the elements on the periodic table by atomic number In1911

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4
Q

Group

A

Vertical

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5
Q

Period

A

Horizontal

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6
Q

Metal

A

Located to the left of the zig zag

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7
Q

Nonmetal

A

Located to the right of the zig zag

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8
Q

Metalloid

A

Located along the zig zag line

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9
Q

Location of alkali metals

A

Group 1

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10
Q

Alkali properties

A

Silvery
Soft
Very reactive
React strong with water

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11
Q

Location of Alkaline earth metal

A

Group 2

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12
Q

Alkaline earth metal properties

A

Harder and denser
Higher melting points
Less reactive

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13
Q

Transition metals

A

D block elements

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14
Q

Why does the D block contain 10 groups

A

There are 5 d orbitals and each contain 2 electrons

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15
Q

Location of halogen

A

Group 17

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16
Q

Halogen properties

A

Most reactive of the nonmetals

Reactive with most levels to form salts

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17
Q

Location of noble gases

A

Group 18

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18
Q

What is the arrangement of noble gases

A

Stable

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19
Q

Inner transition metals

A

Lanthides amd actinides

Groups 6 and 7

20
Q

How is the periodic law demonstrated within groups of the periodic table

A

Elements in a group have similar properties

21
Q

Why are elements not in strict increasing order

A

They are in order of the atomic number, not the atomic mass

22
Q

What info is recorded on the periodic table

A

Atomic number and mass, element name, symbol, and on some you can find the electron configuration

23
Q

How could you organizes elements according to the trends

A

Make predictions

24
Q

How is the periodic table periodic

A

Properties of the elements occur periodically

25
Q

Who discovered periodic law

A

Mendeleev

26
Q

Who established atomic numbers as the basis for organizing

A

Mosley

27
Q

Three sets of elements that has been added since mendeleevs time

A

Helium, krypton, xenon

28
Q

Why are electrons important

A

They find the elements chemically properties

29
Q

Why do elements in the same group have similar properties

A

They have similar electron configurations

30
Q

Into how many blocks is the table divided and what are they called

A

4 blocks,

S,p,d,f

31
Q

What does each block represent

A

The energy level and sub level that is being filled with electrons

32
Q

Why does the s block span two groups of elements

A

S orbitals only hold two electrons

33
Q

Group configuration of each element in group 1

A

Ns1

34
Q

Group configuration of each element in group 2

A

S2

35
Q

Ending electron configuration of the element in period 3, group 1

A

3s1

36
Q

Why does the p block span six groups

A

3p orbitals hold 6 electrons

37
Q

Why are there no p block elements in period 1

A

P orbitals don’t start until the 2nd energy level

38
Q

Ending electron configuration of each element in group 14

A

Ns2np2

39
Q

In what period does the first d energy sublevel appear

A

Period 4

40
Q

In what period does the first f energy sublevel appear why

A

6 because that is where they fall in terms of electrons going in to atoms

41
Q

Why are members of group 18 unreactive

A

There is a stable arrangement of electrons

42
Q

Determine the group, period, and block for the following elements
1s1
[Ne]3s23p1

A

1s1- s block, group 1, period 1

[Ne]3s2 3p1- p block, group 13, period 3

43
Q

Describe the relationship between atomic radio and atomic numbers

A

As atomic number increases the atomic radii decreases

44
Q

What are the smallest and largest first ionization energies

A

Smallest- Fr

Largest- He

45
Q

If an element has a low ionization energy is it easy or hard to remove an electron? Reactive or unreactive?

A

Easier to remove and will be reactive

46
Q

What happens to a numeral atom if it loses one electron

A

It becomes positive

47
Q

Why do the first two elements in the first period not have ionic radii

A

Hydrogen- too small

Helium- doesn’t form ions

48
Q

How can you figure out the charge of an ion

A

Charge = protons - electrons

Honors chemistry (11 decks)

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