Periodic Table Trends

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1

What did John Newlands contribute?

Discovered the Law of Octaves

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2

What did Dmitri Mendeleev contribute?

Produced 1st periodic table w/ all known elements. Predicted properties of undiscovered elements. Grouped by similar properties and arranged by increasing atomic mass.

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3

What did Henry Moseley contribute?

Showed atomic # should be the basis for arranging elements to eliminate discrepancies.

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4

Periodic Law

Repeating physical and chemical properties of elements change periodically with the atomic #.

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5

Valence Electrons

The outermost electrons in an atom.

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6

Which electrons partake in chemical reactions?

Valence Electrons

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7

Groups

Vertical columns on the periodic table.

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8

What explains why similar properties appear on the periodic table?

Electron Configurations

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9

What determines chemical properties?

The number of valence electrons.

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10

Period

Horizontal row on the periodic table.

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11

Electron Shielding

Valence electrons are shielded for nucleus by inner electrons.

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12

What weakens the strength of attraction between the nucleus and valence electrons?

Electron Shielding

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13

During electron shielding, is the repulsion between the inner and outer electrons?

Yes, the like charges cause them to repel.

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14

What is the trend for electron shielding across a group?

Increases down a group since the energy levels are increasing.

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15

What is the trend for electron shielding across a period?

Remains constant

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16

Effective Nuclear Charge

The strength of attraction between protons in the nucleus and the valence electron with shielding electrons taken into account.

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17

What is the trend for ENC across a group?

Decreases down groups; due to increase in distance and shielding electrons

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18

What is the trend for ENC across periods?

Increases across periods; due to additional protons in the nucleus without a change in the electron shielding

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19

Atomic Radius

Size of the atom; electrons occupy most of the volume

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20

Why is atomic radius hard to calculate?

Electrons are located in “clouds” with no definite boundaries.

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21

What is the trend for atomic radius across a group?

Increases down a group; due to electrons occupying additional energy levels which makes the atom bigger.

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22

What is the trend for atomic radius across a period?

Decreases across a period; additional protons pull electrons closer making the atom smaller.

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23

Are cations smaller or larger than their neutral atom?

smaller; due to loss of electrons

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24

Are anions smaller or larger than their atoms?

larger; due to gain of electrons

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25

Ionization Energy

Energy needed to remove an electron from a neutral atom or an ion.

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26

What is the trend for ionization energy across a group?

Decreases down a group; due to # of occupied energy levels and electron shielding

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27

What is the trend for ionization energy across a period?

Increases across a period; addition protons attract electrons.

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28

Electronegativity

An atom’s attraction for electrons when bonded to another atom.

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29

What element has the highest electronegativity?

Fluorine

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30

Do elements with higher electronegativity values hold electrons closer when sharing with another?

Yes

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31

What is the trend for electronegativity across a group?

Decreases; due to additional energy levels and electron shielding.

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32

What is the trend for electronegativity across a period?

Increases; due to additional protons

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33

Electron Affinity

Energy change occurring when a neutral atom attracts an electron

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34

What is the trend for electron affinity across a group?

Decreases due to electron shielding and a decrease in effective nuclear charge.

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35

What is the trend for electron affinity across a period?

Increases due to an increases in effective nuclear charge.

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36

What groups are part of the main-group elements?

1, 2 and 13-18

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37

What are some properties of metals?

Lusters, good conductors, ductile, malleable, varying melting points, form positive ions, can be mixed with other metals to form alloys

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38

Are alloy properties different than pure metals?

Yes

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39

Where are metals located on the periodic table?

Located to the left of the red staircase; metalloids border the red staircase

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40

What are some properties of nonmetals?

Rarely have luster, gases are room temp., not malleable or ductile, poor conductors, exist as diatomic molecules in elemental form, form negative ions, combine w/ nonmetals to form covalent bonds

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41

Where are nonmetals located on the periodic table?

Located to the right of the red staircase; metalloids border red staircase

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42

Metalloids

Properties of metals and nonmetals

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43

What are some characteristics of metalloids?

look metallic, brittle, not malleable or ductile, not good conductors

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44

Where are metalloids found on the periodic table?

Bordering the red staircase

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45

Which group is the alkali metals?

Group 1

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46

How are alkaline solutions formed?

Alkali metals react with water to form alkaline solutions.

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47

What make alkali metals very reactive?

They only have one valence electron which they want to lose.

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48

Why are alkali metals stored in oil?

They have a high reactivity with water and oxygen in the air.

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49

What are some characteristics of the alkali metals?

soft, easily cut, good conductors

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50

What is the most reactive metal?

Francium

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51

Which group is the alkaline earth metals?

Group 2

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52

Why are alkaline earth metals highly reactive?

They have 2 valence electrons which they want to lose.

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53

How are alkaline earth metals found in nature?

Found combined with other elements

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54

What are some characteristics of alkaline earth metals?

harder, higher melting point than alkali metals, good conductors

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55

Which group are the halogens?

Group 17

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56

Which is the most reactive group of nonmetals?

Halogens

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57

Where are Halogens found?

In sea water and rock’s of the Earth’s crust.

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58

What is the rarest naturally occurring elements?

Astatine

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59

How are cations formed?

A loss of electrons

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60

How are anions formed?

A gain of electrons

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61

What group are noble gases?

Group 18

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62

Why do noble gases have a low reactivity?

They have a full valence shell.

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63

Which sublevel contains the transition metals?

d-block

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64

Do transition metals have identical or unidentical valence electron configurations?

Unidentical

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65

What is the most common element in nature?

Hydrogen; highly reactive and unique

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66

What orbitals do lanthanides fill?

4f orbitals

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67

What orbitals do actinides fill?

5f orbitals

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68

What are some properties of actinides?

unique and radioactive, unstable nuclei breaks down and releases radioactive waves

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69

Transuranium Elements

Man-made (synthesized) elements.

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70

Law of Octaves

When elements are arranged in increasing order of atomic mass, the 8th element resembles the 1st in physical and chemical properties.

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71

Periodicity

Trends repeated after certain elements when the elements are arranged by atomic number

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72

Which elements form cations?

Elements to the left of the red staircase

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73

Which elements for anions?

Elements to the right of the red staircase.

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