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Chemistry > Periodic Trends > Flashcards

Periodic Trends Flashcards

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1
Q

Row

A

Period

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2
Q

Properties of Valence Electrons (3)

A
  • determines the chemical properties of the elements
  • the electrons on the highest energy level
  • are related to the group number of the element
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3
Q

Period

A

Row

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4
Q

Column

A

Group (not including transition elements)

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5
Q

What is the pattern of elements in the same group?

A

they both have the same number of valence electrons

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6
Q

What does the electron-dot symbol indicate?

A

the valence electrons as dots around the symbol of the element.

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7
Q

What does the electron-dot symbol show?

A

the number of valence electrons an element has

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8
Q

Relationship between elements of groups and electron-dot symbol

A

In a group, all the electron-dot symbols have the same number of valence electrons (dots).

ex) all elements in group 2 have 2 dots

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9
Q

The three periodic trends

A

Atomic Radius, Ionization E, Electron Affinity

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10
Q

Atomic Radius

A

actual size of atom measured from nucleus to valence e-’s

(Distance from nucleus to outermost shell)

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11
Q

Ionization Energy

A

Energy required to overcome the attraction from the nucleus and REMOVE an e-

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12
Q

Electron Affinity

A

potential energy change of the atom when an electron is added to a neutral atom to form a negative Ion

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13
Q

Shielding Effect

A

trends ACROSS the periodic table usually deal with electrons being added to the SAME energy level

trends DOWN a group usually deals with adding electrons to an INCREASING number of energy levels

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14
Q

Atomic Size

A

The distance from the nucleus to the valence electrons

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15
Q

How is atomic size described as?

A

by using the atomic radius

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16
Q

Patterns of Atomic Radius within a Group

A

atomic radius INCREASES when going DOWN a group

atomic radius DECREASES when going ACROSS a period

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17
Q

The element needs to be in what state for Ionization energy to occur?

A

gas

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18
Q

The _____ the radius is the _____ it is to remove an electron

A

bigger, harder

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19
Q

Ionization energies of metals are…

A

low

20
Q

Ionization energies of non-metals are…

A

high

21
Q

What does an increase in Ionization energy show?

A

tells that the element is taking on the electron configuration of the nearest noble gas

(breaking into a stable gas structure)

22
Q

Metals are what kind of ion?

A

cation

23
Q

Non-metals are what kind of ion?

A

anion

24
Q

Positive Metal Cations are how large compared to the neutral atoms?

A

smaller than the neutral atoms from which they form from

25
Q

Negative Nonmetal Anions are how large compared to the neutral atoms?

A

larger than the neutral atoms from which they form from

26
Q

Electronegativity

A

ability of an atom to attract electrons from other atoms

27
Q

The more ____ the electron affinity the more __ the electron addition process is

A

negative, favourable

28
Q

What unit is electron affinity in?

A

kJ/mol

29
Q

Electron Affinity Trend

A

Metals are LOW
Non-metals are HIGH

30
Q

What letter is used for representative elements?

A

A

31
Q

What are the representative elements?

A

elements from 1A to 8A

32
Q

What elements does the A represent?

A

representative elements

33
Q

What letter is used to represent transition elements?

A

B

34
Q

What letter is B used to represent?

A

transition elements

35
Q

Group numbers can also refer to (not a or b)…

A

the numbers in columns 1-18, left to right

36
Q

What are representative elements known by?

A

common names

37
Q

What common names do the groups go by?

A

1A - Alkali metals
2A - Alkaline-earth metals
3A-6A - No common names
7A - Halogens
8A - Noble Gas

38
Q

Alkali Metals

A

Group 1A (1) which includes lithium, sodium, and potassium and forms a basic solution

39
Q

Where are metals located?

A

left

40
Q

Where are non-metals located?

A

right

41
Q

Where are semi-metals located?

A

located along the heavy zigzag line between the metals and nonmetals

42
Q

Properties of Metals

A

shiny and ductile (can bend into shapes)

are GOOD conductors of heat and electricity

43
Q

Properties of Nonmetals

A

dull, brittle (crack/break easily)

POOR conductors of heat and electricity

44
Q

Properties of Metalloids/Semimetals

A

BETTER conductors than non-metals, but NOT AS GREAT as metals

used as semiconductors and insulators

45
Q

The metalloids section in the periodic table

A

B, Si, Ge, As, Sb, Te, Po, At

Chemistry (8 decks)

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