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Chemistry Test - Periodic Trends Flashcards

1
Q

What information is used to organize the modern periodic table?

A
  • Atomic number
  • Valence shells
  • Element properties
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2
Q

How does atomic mass relate to the atomic number?

A

Atomic number = mass - neutrons

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3
Q

What does periodic mean?

A

Periodic means a repeating pattern.

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4
Q

What properties are common to the left side of the periodic table you made? What properties are common to the right side of the periodic table you made?

A

Left: soft, shiny metals that react with oxygen and water.
Right: Non-Metals and gases.

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5
Q

Where are the Akali Metals?

A

First Column

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6
Q

Where are the Alkaline Earth Metals?

A

Second Column

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7
Q

Where are the Halogens?

A

Second column on the right side (F, Cl. Br, I)

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8
Q

Where are the Noble gases?

A

Furthest right column.

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9
Q

Which element in each of the following groups has the largest atomic radius? (Halogens, Alkali Metals, Noble Gases)

A

a) Halogens - Iodine
b) Alkali Metals - Francium
c) Noble Gases - Radon

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10
Q

Arrange the following atoms in order of increasing atomic radius (smallest to largest): K, Rb, Cs, F, Li, C

A

Li, C, F
K, Rb, Cs

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11
Q

Atomic Radius Definition:

A

A measurement of the size of an ion, usually expressed in picometers (pm); the distance from the centre of an ion to the outermost (valence) electrons.

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12
Q

Across a Row Atomic Radius Increases:

A

From right to left.

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13
Q

Across a Row Atomic Radius Decreases:

A

From left to right

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14
Q

Atomic Radius Row Example for Smallest Radius: Li or F?

A

F is the smallest as it is towards the right side of the periodic table. Atoms further on the right of the periodic table have more protons to attract the electrons in. Therefore, making the atomic radius smaller as the electrons are pulled closer to the nucleus.

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15
Q

Atomic Radius Row Example for Biggest Radius: S or Mg?

A

Mg is the biggest radius as it is towards the left side of the periodic table. Atomics further on the left of the periodic table have fewer protons to attract the electrons in. Therefore, making the atomic radius bigger as the electrons are further away from the nucleus.

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16
Q

Template for Atomic Radius Row examples:

A

( ) is the (smallest/biggest) as it is towards the (right/left) of the periodic table. Atoms further on the (right/left) of the periodic table have (more/fewer) protons to attract electrons in. Therefore, making the atomic radius (smaller/bigger) as the electrons are (pulled closer to/further away from) the nucleus.

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17
Q

Column Atomic Radius Increases:

A

As you go down a column.

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18
Q

Column Atomic Radius Decreases:

A

As you go up a column.

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19
Q

Atomic Radius Column Example for Smallest Radius: Sr or Be?

A

Be is the smallest as it is higher up in the column. Atoms higher up have fewer shells and therefore, are smaller.

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20
Q

Atomic Radius Column Example for Biggest Radius: O or Se?

A

Se is the biggest as It is lower down in the column. Atoms lower down have more shells and therefore, are bigger.

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21
Q

Template for Atomic Radius Column:

A

( ) is the (smallest/biggest) as it is (higher up/lower down) in the column. Atoms (higher up/lower down) have (fewer/more) shells and therefore, are (smaller/bigger).

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22
Q

Ionization Energy Definition:

A

The quantity of energy required to remove an electron from an atom or ion in the gaseous state.

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23
Q

Across a Row Ionization Energy Increases:

A

To the right.

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24
Q

Across a Row Ionization Energy Decreases:

A

To the left.

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25
Q

Ionization Energy Row Example for Lowest I.E.: Na or P?

A

Na is further to the left so it has less protons than P. Therefore, electrons are attracted less strongly and Ionization Energy is lower.

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26
Q

Ionization Energy Row Example for Highest I.E.: Be or O?

A

O is further to the right so it has more protons than Be. Therefore, electrons are attracted more strongly and Ionization Energy is higher.

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27
Q

Template for Ionization Energy Row:

A

( ) is further to the (left/right) so it has (less/more) protons than ( ). Therefore, electrons are attracted (more/less) strongly and Ionization Energy is (lower/higher).

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28
Q

Column Ionization Energy Increases:

A

Up a column.

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29
Q

Column Ionization Energy Decreases:

A

Down a column.

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30
Q

Ionization Energy Column Examples for Highest I.E.: Sr or Be?

A

Be is higher in the column, giving it a smaller radius and thus, less inner shielding electrons. This makes the energy valence electrons closer to the protons, with less electrons in the way. Therefore, creating a higher attraction, and a higher Ionization Energy, making the electrons harder to remove.

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31
Q

Ionization Energy Column Example for Lowest I.E.: O or Se?

A

Se is lower in the column, giving it a larger radius and thus, more inner shielding electrons. This makes the energy valence electrons further away from the protons, with more electrons in the way, Therefore, creating a lower attraction, and a lower Ionization Energy, making the electrons easier to remove.

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32
Q

Template for Ionization Energy Column:

A

( ) is (lower/higher) in the column, giving it a (larger/smaller) radius and thus, (more/less) inner shielding electrons. This makes the energy valence electrons (closer to/further away from) the protons, with (more/less) electrons in the way. Therefore, creating a (lower/higher) attraction, and a (lower/higher) Ionization Energy making the electrons (easier/harder) to remove.

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33
Q

? is colourless in an acid and pink in a base

A

Phelophalen is colourless in an acid and pink in a base

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34
Q

? react by losing electrons

A

Metals react by losing electrons

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35
Q

? is the energy required to remove the electron

A

Ionization energy is the energy required to remove the electron

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36
Q

Anything that lowers the ? allows the electron to be removed more easily and gives it a bigger reaction

A

Anything that lowers the ionization energy allows the electron to be removed more easily and gives it a bigger reaction

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37
Q

Write out the full reaction for either Li or K, or Rb, or Cs as was done in the example with Na in the video.
Sodium + Water -> Sodium Hydroxide + Hydrogen Gas
2Na(s) + 2HOH(l) -> 2NaOH(aq) + 1H2(g)

A

Potassium + Water -> Potassium Hydroxide + Hydrogen Gas
2K(s) + 2HOH(l) -> 2KOH(aq) + 1H2(g)

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38
Q

The word format for column 1 (Alkali metals) reactions with water?

A

Alkali Metal + Water -> Alkali Metal Hydroxide + Hydrogen Gas

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39
Q

The elemental format for column 1 (Alkali metals) reactions with water?

A

2Alkali Metal Symbol(s) + 2HOH(l) -> 2Alkali Metal Symbol OH(aq) + 1H2(g)

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40
Q

What left each of the metals that caused the reaction?

A

Electrons.

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41
Q

Use the ideas of ionization energy and shells to explain why Li was the least reactive, Na was more reactive and K was the most reactive of the elements that we tested in class. [4]
Hints
a) How many shells does Li have and does this make the radius Big or medium or small?
b) Does this put the valence electron close to or far away from the protons in the nucleus?
c) Are there many inner shielding electrons between the valence electron and the nucleus? What does this do to the attraction between the Valence and the nucleus?
d) What do the above do to the ionization energy and the reactivity?

A
  • Lithium has the smallest number of shells and therefore the smallest radius.
  • This means the valence electron is the closest to the protons and is attracted more strongly.
  • Lithium also has the fewest inner shielding electrons blocking the valence electron from seeing the protons.
  • Therefore the valence electron is attracted more.
    For both reasons, the electron is harder to remove, and the Ionization energy is highest. Since metals react by losing electrons, Li is the least reactive.
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42
Q

Which element from the same column (Alkali metals) would be the most reactive? Why?

A

Francium would be the most reactive because…
- Francium has the biggest number of shells and therefore the biggest radius.
- This means the valence electron is the furthest to the protons and is attracted the least strongly.
- Francium also has the most inner shielding electrons blocking the valence electrons from seeing the protons.
- Therefore the valence electron is attracted less.
For both reasons, the electron is easier to remove, and the Ionization energy is the lowest. Since metals react by losing electrons, Fr is the most reactive.

43
Q

Template for asking what element in each column would be the most/least reactive

A
  1. ( ) would be the (least/most) reactive because…
    • ( ) has the (smallest/biggest) number of shells and therefore the (smallest/biggest) radius.
    • This means the valence electron is the (closest/furthest) to the protons and is attracted (more/the least) strongly.
    • ( ) also has the (fewest/most) inner shielding electrons blocking the valence electron from seeing the protons.
    • Therefore the valence electron is attracted (more/less).

6.For both reasons, the electron is (harder/easier) to remove, the Ionization energy is the (highest/lowest). Since metals react by losing electrons, ( ) is the (least/most) reactive.

44
Q

What gas was produced by each of the reactions and what ignited the gas for the more reactive elements?

A

Hydrogen gas was produced by each of the reactions and the heat from the reaction ignited the gas for the more reactive elements.

45
Q

Why did the phenolphthalein turn pink in the water after each element had reacted with the water?

A

The phenolphthalein turned pink in the water after each element reacted with the water because you made a base.

46
Q

The Alkaline Earth Metals are in Column #?

A

2

47
Q

The number of Valence Electrons Alkaline Earth Metals have is?

A

2

48
Q

Compared to the Alkali Metals in Column 1, Alkaline Earth metals have ? more proton.

A

1

49
Q

Based upon the number of protons and shells, state whether the column 2 metals will be more or less reactive than the column 1 metals right beside them.

A

Calcium will be less reactive than magnesium because as you go across a row protons increase, increasing ionization energy, decreasing reactivity

50
Q

What Gas was formed when Magnesium and Calcium were placed in water? How do you know?

A

Hydrogen gas was produced - we know because the burning splint gave a “poof” or a “pop.”

51
Q

What type of substance Acid or Base was formed when the metals were placed in water? How do you know?

A

A base was produced - we know because the phenolphthalein turned pink.

52
Q

What is the name and formula of the metal products formed by the reactions?

A

Calcium + Water -> Calcium Hydroxide + Hydrogen - Ca(OH)2
Magnesium + Water -> Magnesium Hydroxide + Hydrogen - Mg(OH)2

53
Q

What was the identity of the Calcium Hydroxide solution? What result in this lab confirmed this to you?

A

Lime Water - Mr. Draggert breathed CO2(g) into the Ca(OH)2 and it turned cloudy white.
A positive test for CO2(g) is that when mixed with Limewater, limewater turns cloudy white. Therefore, Ca(OH)2 is limewater.

54
Q

Write the Balanced Chemical Equation for the reaction of Calcium and water.

A

1Ca(s) + 2HOH(l) -> 1Ca(OH)2(aq) + 1H2(g)

55
Q

The word format for column 2 (Alkaline Earth metals) reactions with water?

A

Alkaline Earth Metal + Water -> Alkaline Earth Metal Hydroxide + Hydrogen Gas

56
Q

The elemental format for column 2 (Alkaline Earth metals) reactions with water?

A

1Alkaline Earth Metal Symbol(s) + 2HOH(l) -> 1Alkaline Earth Metal Symbol (OH)2(aq) + 1H2(g)

57
Q

Why is Mg less reactive than Na and Ca less reactive than K? Remember, I did not let you use the Alkali Metals (column 1) and K actually caught on fire. I let you use the Alkaline Earth Metals and Ca right beside K did not catch on fire.

A

Mg is less reactive than Na, and Ca is less reactive than K because they have a larger atomic radius, no protons blocking, and thus, lower ionization energy.

58
Q

Why did Mg react less than Ca?

A

Calcium has a bigger atomic radius - more protons blocking the valence electron - and is further down the column so it has lower ionization energy as the valence electrons are further away, therefore, lower attraction.

59
Q

What do the words Alkali and Alkaline from the column titles indicate? How did your lab results verify this?

A

They indicate/mean base. So when you stick one of those metals in water you will get a base.

60
Q

Electronegativity Definition:

A

The ability of an individual atom when Bonded to attract electrons to itself. The Electronegativity Values of the atoms are found right below the atomic Number on the left-hand side of the Element boxes on the Periodic Table

61
Q

Across a Row Electronegativity Increases:

A
  • Same as I.E and E.A. The Electronegativity (E.N.) increases as you go from Left to Right across a row.
  • As you move right across a row the number of protons increases. This increases the effective positive nuclear charge that can attract a new electron into the valence shell when bonding. Therefore the ability of an atom to attract an electron in a bond (E.N.) increases towards the right.
62
Q

Across a Row Electronegativity Decreases:

A
  • Same as I.E and E.A. The Electronegativity (E.N.) decreases as you go from Right to Left across a row.
  • As you move left across a row the number of protons decreases. This decreases the effective positive nuclear charge that can attract a new electron into the valence shell when bonding. Therefore the ability of an atom to attract an electron in a bond (E.N.) decreases towards the right
63
Q

Electronegativity Row Example for Lowest Electronegativity: Li or F?

A

Li has the lowest electronegativity because it is furthest left, meaning it has less protons to attract bonding electrons than F aka Li has a lower effective positive nuclear charge to attract electrons into its valence shell while bonding. Therefore Li has the lower Electronegativity.

64
Q

Electronegativity Row Example for Highest Electronegativity: S or Mg?

A

S has the highest electronegativity because it is the furthest right, meaning S has more protons to attract bonding electrons than Mg aka S has a higher effective nuclear charge to attract electrons into its valence shell while bonding. Therefore S has the higher Electronegativity

65
Q

Template for Electronegativity Row Examples:

A

( ) has the (lowest/highest) electronegativity because it is furthest (left/right), meaning it has (less/more) protons to attract bonding electrons than ( ) aka ( ) has a (lower/higher) effective nuclear charge to attract electrons into its valence shell while bonding. Therefore ( ) has the (lower/higher) Electronegativity.

66
Q

Column Electronegativity Increases:

A

Same as I.E. and E.A Electronegativity increases as you go up a column.
- Elements at the top of a column have less shells, smaller radius placing the valence shell closer to the nucleus.
As well less inner shielding electrons between the valence shell and the nucleus.
- Therefore, elements at the top have a higher ability to attract new electrons thus a higher electronegativity

67
Q

Column Electronegativity Decreases:

A

Same as I.E. and E.A., Electronegativity decreases as you go down a column.
- Elements at the bottom of a column have more shells and thus a bigger radius placing the valence shell further away from the nucleus.
As well, they have more inner shielding electrons
- Therefore, elements at the bottom have a lower ability to attract new electrons a lower electronegativity

68
Q

Electronegativity Column Example for Lowest Electronegativity: Sr or Be?

A

Sr has the lowest Electronegativity because…
- It has more shells, thus, a bigger atomic radius and placing its valence shell further away from the nucleus.
- As well it has more inner shielding electrons between the valence shell and the nucleus blocking the valence shell from seeing the protons.
Therefore for both reasons, Sr has a lower ability to attract electrons to its valence shell while bonding and thus, a lower Electronegativity.

69
Q

Electronegativity Column Example for Highest Electronegativity: O or Se?

A

O has the highest Electronegativity because…
- It has less shells, thus, a smaller atomic radius and placing it’s valence shell closer to the nucleus.
- As well it has less inner shielding electrons between the valence shell and the nucleus blocking the valence shell from seeing the protons.
Therefore for both reasons, O has a higher ability to attract electrons to its valence shell while bonding and thus a higher Electronegativity.

70
Q

Template for Electronegativity Column Examples:

A

Template for Electronegativity Column Examples:
( ) has the (lowest/highest) Electronegativity because..
- It has (more/less) shells, thus, a (bigger/smaller) atomic radius and placing its valence shell (further away from/closer to) the nucleus.
- As well it has (more/less) inner shielding electrons between the valence shell and the nucleus blocking the valence shell from seeing the protons.
Therefore for both reasons, ( ) has a (lower/higher) ability to attract electrons to it’s valence shell while bonding and thus a (lower/higher) Electronegativity.

71
Q

Metals react by ? electrons.

A

Losing

72
Q

The most important property is the one that describes how much energy is needed to remove an electron from the atom. This is known as the ?

A

Ionization Energy

73
Q

Non-metals on the other hand react by ? electrons.

A

Gaining

74
Q

The most important property describes the ability of an atom to attract electrons within a bond. This is known as: ?

A

Electronegativity

75
Q

Anything that raises the electronegativity: ? the reactivity of non-metals.

A

Increases

76
Q

Is Fluorine super reactive? How do the observations help you determine this? How does the fact that no heat had to be added help you determine this?

A

It is super reactive because it instantly sets everything on fire and you didn’t even have to heat it up it instantly just did that because it is that reactive.

77
Q

Are Fluorine and Chlorine super reactive? How do you know?

A

Yes because they react instantly.

78
Q

Why did he not have to add heat to the Fluorine gas but had to add heat (light with a spark) to Chlorine Gas to get it to burn with Hydrogen? What does this indicate about the reactivity of Chlorine vs. Fluorine?

A

Chlorine is very reactive just not as reactive as fluorine because it needed some heat while fluorine did not.
- Chlorine is a bit less reactive than Fluorine because the scientist had to add heat to get it to instantly react.

79
Q

The term valency of one for the halogens means a charge of ?

A

-1

80
Q

What do the observations indicate about the reactivity of Chlorine vs. Fluorine? How do you know?

A

Chlorine is a bit less reactive than Fluorine.
Fluorine = most reactive, reacted faster without heat.
Chlorine = less reactive, reacted slower with heat

81
Q

Fluorine reacted instantly and Chlorine reacted fairly quickly. Bromine reacted more slowly. What does this indicate about the reactivity of Bromine compared to Chlorine and Fluorine?

A

Bromine is less reactive than Fluorine and Chlorine because it reacts more slowly.

82
Q

Iodine reacted even more slowly and had to be warmed up. What does this indicate about the reactivity of Iodine compared to Br, Cl, and F?

A

Iodine is the least reactive in comparison to Br, Cl, and F because it reacted the slowest and needed to be heated up.

83
Q

Therefore the order of reactivity for the Halogens is

A

Highest
F Faster
Cl
—————————————-
Br
I Slower
Lowest

84
Q

Using the Number of Shells, Atomic Radius, and Electronegativity, explain: Why Fluorine is so much more reactive (it is the most reactive) than all of the other Halogens.

A
  1. Fluorine has the least number of shells. Therefore it has the smallest atomic radius.
  2. Therefore the valence shell is closest to the positive nucleus.
  3. F has the least number of inner shielding electrons between the valence shell and the nucleus.
  4. Therefore the attraction between the protons and new electrons for F is the highest. Therefore the electronegativity is highest.
  5. Since non-metals react by gaining electrons, F is the most reactive.
85
Q

Using the Number of Shells, Atomic Radius, and Electronegativity, explain: Why Iodine is so much less reactive (it is the least reactive) than all of the other Halogens.

A
  1. Iodine has the most number of shells. Therefore it has the biggest atomic radius.
  2. Therefore the valence shell is the furthest away from the positive nucleus.
  3. I has the most number of inner shielding electrons between the valence shell and the nucleus, blocking the new electrons from seeing the protons.
  4. Therefore the attraction between the protons and new electrons for I is the lowest. Therefore the electronegativity is the lowest.
  5. Since non-metals react by gaining electrons, F is the least reactive.
86
Q

Template for Using the Number of Shells, Atomic Radius, and Electronegativity, explain Halogen reactivity

A
  1. ( ) has the (most/least) number of shells. Therefore it has the (biggest/smallest) atomic radius.
  2. Therefore the valence shell is the (closest to/furthest away from) the positive nucleus.
  3. ( ) has the (most/least) number of inner shielding electrons between the valence shell and the nucleus, (if most - blocking the new electrons from seeing the protons.)
  4. Therefore the attraction between the protons and new electrons for ( ) is the (highest/lowest). Therefore the electronegativity is the (highest/lowest).
  5. Since non-metals react by gaining electrons, ( ) is the (most/least) reactive.
87
Q

Write the word and balanced chemical equation for Barium + Water.

A

Barium + Water -> Barium Hydroxide + Hydrogen Gas
1Ba(s) + 2HOH2(l) -> 1Ba(OH)2(aq) + 1H2(g)

88
Q

How do you know a base is made?

A

The phenolphthalein turned pink.

89
Q

What gas was made? How do you know?

A

H2(g), the burning splint “popped”

90
Q

What does Alkaline in the name Alkaline Earth metal mean?

A

It means Base.

91
Q

Write the word and balanced chemical equations for Cesium + Water.

A

Cesium + Water -> Cesium Hydroxide + Hydrogen Gas
2Cs(s) +2HOH(l) -> 2CsOH(aq) + 1H2(g)

92
Q

Why did the phenolphthalein turn pink?

A

The reaction made a base.

93
Q

What gas was made? What ignited it for the ones that caught on fire?

A

Hydrogen gas - H2(g) and the heat the reaction produced.

94
Q

What does Alkali mean in Alkali metals?

A

Base.

95
Q

Why can Chlorine and Bromine be used to clean swimming pools but Iodine and Fluorine can’t?

A

Note: Non-Metals react by gaining electrons.
As you go down the column, the # of shells and therefore the radius increases. This puts the valance shell further away.
As you go down the column, the number of inner shielding electrons increases, blocking the protons more.
Therefore Fluorine has the most attraction and highest E.N. it is so reactive that it would burn your skin and eyes.
Chlorine and Bromine have medium attraction, therefore they clean but are not too harsh on the skin and eyes. Bromine is just a bit bigger with a few more inner shielding electrons. Therefore, it is less reactive and gentler.
Iodine is so big with so many inner shielding electrons that it has the least attraction and a low E.N. Therefore, it is not reactive enough to clean the pool.

96
Q

Which has the smallest Atomic Radius? Why? - Na Al Cl

A

Cl is furthest to the right with the most protons to attract electrons in.

97
Q

Which has the smallest Atomic Radius? Why? - Ga In Tl

A

Ga is the furthest up in the column with the least number of shells.

98
Q

Which has the largest atomic radius? Why? - La Pt Rn

A

La is furthest to the left which means it has fewer protons to pull in the electrons.

99
Q

Which has the largest atomic radius? Why? - C Sn Pb

A

Pb is at the bottom so it has the most shells.

100
Q

Which has the highest Ionization Energy? Why? - Mg Sr Ra

A

Mg has less shells therefore, is clsoeer to protons which means a higher attraction. Mg also has less inner shielding electrons blocking protons which also means a higher attraction. Therefore, higher ionization energy.

101
Q

Which has the highest Ionization Energy? Why? - Al P Cl

A

Cl is furthest to the right therefore, it has the most protons to attract electrons in. Therefore, highest ionization energy.

102
Q

Tin (Sn) is a great metal to use for soup cans, Rb would be awful. Using I.E. explain why Tin is often used for soup cans and Rb is never used.
What are 3 bad things that would happen if Rb was used.

A

Sn is furthest to the right with more protons to attract electrons. Therefore, it is harder to remove valence electrons anf I.E is higher. Since metals react by losing electrons, therefore Sn will not react and is safe to use.
Three bad things that would happen are …
- Rb would produce H2(g) and heat = a fire
- Which would create a corrosive base in soup
- The tin would disappear and base would leak everywhere

103
Q

Three bad word problems things

A
  • ( ) would produce H2(g) and heat = a fire
  • Which would create a corrosive base in ( )
  • The (metal) would disappear and base would leak everywhere

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