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Unit 4 Chemistry: Periodic Trends Flashcards

1
Q

Where are metals located on the Periodic Table?

A

Left side

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2
Q

Where are the nonmetals located on the Periodic Table?

A

Right side

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3
Q

What are some properties of metals?

A

Malleable, Ductile, Lustrous, good conductors

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4
Q

What are some properties of nonmetals?

A

Non-lustrous, brittle, poor conductors

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5
Q

Who first came up with the periodic table?

A

Mendeleev

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6
Q

How did Mendeleev organize the elements?

A

Increasing atomic mass

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7
Q

Who’s organization of the elements on the periodic table do we use today?

A

Moseley

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8
Q

How did Moseley organize the elements?

A

Increasing atomic number

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9
Q

What does the periodic law state?

A

When elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and chemical properties.

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10
Q

What is a period?

A

Horizontal rows across the periodic table.

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11
Q

What is a group?

A

Vertical columns down the periodic table.

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12
Q

What do elements in the same group have?

A

Similar properties

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13
Q

What are groups numbered?

A

1-18

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14
Q

What do elements in the same period have and not have?

A

They don’t have similar properties, but they have the same number of occupied energy levels.

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15
Q

What are periods numbered?

A

1-7

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16
Q

What are the s and p blocks called?

A

Representative elements

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17
Q

What is the d block called?

A

Transition metals

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18
Q

What is the f block called?

A

Inner transtition metals

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19
Q

What are metalloids?

A

Elements that touch the staircase and have properties of both metals and non metals.

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20
Q

What are elements in group 1 called?

A

Alkali Metals

21
Q

What are elements in group 2 called?

A

Alkaline Earth Metals

22
Q

What are elements in group 17 called?

A

Halogens

23
Q

What are elements in group 18 called?

A

Noble Gases

24
Q

What is the atomic radius?

A

1/2 of the distance between the Nuclei of two like atoms.

25
Q

What is the group trend for atomic size?

A

The atomic size will increase due to a greater number of occupied energy levels.

26
Q

What is the period trend for Atomic size?

A

The Atomic size decreases from left to right due to a greater number of protons (increased nuclear charge)

27
Q

What is the shielding effect?

A

The period trend is less pronounced for periods further down the P.T

28
Q

What is ionization energy?

A

The amount of energy required to move an electron from a gaseous atom.

29
Q

What does the ionization energy depend on?

A
  1. Distance between electron and nucleus
  2. Nuclear Charge (# of protons)
30
Q

What is the group trend for I.E?

A

I.E decreases as you go down a group due to a greater # of energy levels.

31
Q

What is the period trend for I.E?

A

I.E increases as you move across a period due to an increased nuclear charge.

32
Q

When is there a very large increase in I.E?

A

When an electron is removed from an atom/ion that is isoelectronic with a noble gas.

33
Q

Cations are always ______ than the neutral atom from which they are made.

A

Smaller

34
Q

The more electrons lost in cations, _____

A

The smaller an ion becomes

35
Q

Anions are always _____ than the neutral atom from which they are made.

A

Larger

36
Q

The more electrons gained in an Anion _____

A

The bigger the ion becomes

37
Q

More electrons than protons result in ______

A

Less attractive force

38
Q

What is electronegativity?

A

The tendency for an element to attract electrons when chemically combined with another element.

39
Q

What element has the highest E.N?

A

Fluorine (4.0)

40
Q

What is the group trend for E.N?

A

E.N decreases as you go down a group because the electrons are less attracted to the nucleus (more energy levels).

41
Q

What is the period trend for E.N?

A

E.N increases as you go across a period because electrons are more attracted to the nucleus due to increased nuclear charge.

42
Q

Which atom has a larger atomic size, Nitrogen or Arsenic?

A

Arsenic

43
Q

Which atom has a smaller atomic size, Vanadium or Manganese?

A

Manganese

44
Q

Which atom has a larger first ionization energy, phosphorus or sulfur?

A

Sulfur

45
Q

Which atom/ion is larger, Mg+2 or Mg?

A

Mg

46
Q

Which atom has the larger electronegativity, Carbon or Flourine?

A

Fluorine

47
Q

Label what element the E.C corresponds to, C=2s^2 2p^6?

A

Neon

48
Q

What is the electron configuration for group 12?

A

d^10

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