$CATEGORY: Science - Khan Academy/5.Periodic Classification of Elements/5.Periodic Classification of Elements--Making Order Out of Chaos-The Modern Periodic Table

//Multiple Choice

What happens to the metallic character as we move down a group in the periodic table?
{
  = Increases
  ~ Decreases
  ~ Remains constant
  ~ First increases, then decreases
}

What happens to the metallic character as we move across a period from left to right?
{
  ~ Increases
  = Decreases
  ~ Remains constant
  ~ First decreases, then increases
}

Which element is the most metallic in Group 1?
{
  ~ Lithium
  ~ Sodium
  ~ Potassium
  = Cesium
}

Which property is directly related to the metallic character of an element?
{
  ~ Ionization energy
  ~ Electronegativity
  = Atomic size
  ~ Electron affinity
}

Which element is the least metallic in Period 3?
{
  ~ Sodium
  ~ Magnesium
  ~ Silicon
  = Chlorine
}

As we move across a period, the tendency to lose electrons __________.
{
  ~ Increases
  = Decreases
  ~ Remains constant
  ~ First increases, then decreases
}

Which of the following is the most metallic?
{
  = Aluminum
  ~ Boron
  ~ Silicon
  ~ Carbon
}

What is the trend of metallic character in Group 17?
{
  = Increases down the group
  ~ Decreases down the group
  ~ Remains constant
  ~ First increases, then decreases
}

Which of the following elements is the least metallic?
{
  ~ Sodium
  ~ Magnesium
  ~ Aluminum
  = Phosphorus
}

Which of these elements shows the most metallic character in Period 2?
{
  = Lithium
  ~ Beryllium
  ~ Boron
  ~ Fluorine
}

//True or False

Metallic character increases across a period. {F}

Metallic character decreases down a group. {F}

Elements with low ionization energy have high metallic character. {T}

Nonmetals are more metallic than metals. {F}

Metallic character is inversely related to electronegativity. {T}

Group 1 elements are highly metallic. {T}

Cesium is more metallic than Sodium. {T}

Metallic character increases with increasing atomic size. {T}

Metallic character is highest in Group 17 elements. {F}

Fluorine has no metallic character. {T}

//Fill in the blanks

The metallic character __________ as we move down a group.
{
  = Increases
  ~ Decreases
  ~ Remains constant
}

The metallic character __________ as we move across a period from left to right.
{
  ~ Increases
  = Decreases
  ~ Remains constant
}

The element with the highest metallic character in Period 3 is __________.
{
  = Sodium
  ~ Magnesium
  ~ Aluminum
}

Metallic character is related to the ability of an element to __________ electrons.
{
  = Lose
  ~ Gain
  ~ Share
}

The metallic character is higher in __________.
{
  = Cesium
  ~ Lithium
  ~ Sodium
}

In Period 2, the element with the least metallic character is __________.
{
  ~ Lithium
  = Fluorine
  ~ Boron
}

The metallic character of elements in Group 1 __________ as we move down the group.
{
  = Increases
  ~ Decreases
  ~ Remains constant
}

The metallic character of elements in Group 17 __________ as we move down the group.
{
  = Increases
  ~ Decreases
  ~ Remains constant
}

As metallic character decreases, the tendency to __________ electrons increases.
{
  ~ Lose
  = Gain
  ~ Share
}

The least metallic element in Group 1 is __________.
{
  = Lithium
  ~ Sodium
  ~ Potassium
}

//Numericals

If the ionization energy of Sodium is 496 kJ/mol and that of Potassium is 419 kJ/mol, which has higher metallic character?
{
  ~ Sodium
  = Potassium
  ~ Both are equal
}

The ionization energy of Lithium is 520 kJ/mol, and that of Cesium is 375 kJ/mol. What is the difference?
{
  ~ 145 kJ/mol
  ~ 245 kJ/mol
  ~ 345 kJ/mol
}

If the atomic radius of Sodium is 186 pm and that of Magnesium is 160 pm, which has higher metallic character?
{
  = Sodium
  ~ Magnesium
}

The electronegativity of Chlorine is 3.0, and that of Sodium is 0.9. Which is more metallic?
{
  ~ Chlorine
  = Sodium
}

The atomic radius of Potassium is 231 pm, and that of Rubidium is 244 pm. Which has higher metallic character?
{
  ~ Potassium
  = Rubidium
}

The metallic character of an element is inversely proportional to its __________.
{
  = Ionization energy
  ~ Atomic size
  ~ Shielding effect
}

The ionization energy of Cesium is 375 kJ/mol. What will be its metallic character compared to Lithium (520 kJ/mol)?
{
  = Higher
  ~ Lower
}

If the atomic size increases, the metallic character __________.
{
  = Increases
  ~ Decreases
  ~ Remains constant
}

The ionization energy of Magnesium is 737 kJ/mol, and that of Calcium is 590 kJ/mol. Which has higher metallic character?
{
  ~ Magnesium
  = Calcium
}

The atomic size of Fluorine is 64 pm, and that of Lithium is 152 pm. Which is more metallic?
{
  ~ Fluorine
  = Lithium
}

//Match the following

Match the following items from Column A with their correct corresponding options from Column B\:
{
  = Across a period -> Metallic character decreases 
  = Down a group -> Metallic character increases
  = Low ionization energy -> High metallic character 
  = High electronegativity -> Low metallic character 
}


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