Chemistry Quiz
Ionization-Increasing- V or Al
Al
Ionization energy is the energy
energy required to remove an electron from a specific atom.
What is first ionization energy?
energy required to remove the first electron from a neutral atom
Of the main group elements,
fluorine has the highest electronegativity (EN = 4.0) and cesium the lowest (EN
Electronegativity values generally increase
from left to right across the periodic table.
Electronegativities generally decrease
from top to bottom of a group.
Moving from left to right across the periodic table,
the ionization energy for an atom increases.
What are valence electrons?
electrons in the outermost energy level
How does it increase?
As the number of protons in the nucleus increases, the electronegativity or attraction will increase. Therefore electronegativity increases from left to right in a row in the periodic table.
How does it decrease?
As you move down a group
What is the octet rule?
Atoms tend to gain, lose or share electrons in order to have a full set of valance electrons in their outermost shell. MOST elements will gain or lose electrons in order to have 8 valence electrons This results in a full s and p sub level!
Explain why the elements in group 1 have low electronegativity values.
Because the metals in group 1 have few valence electrons, they increase their stability by losing electrons, this the electronegativities of metals are lower .
Explain why ionization energy increases as you move left to right
Because the more protons/atomic number in the nucleus makes it harder to remove electrons
These electrons are involved in?
Bonding
Ionization-Increasing-BE or C
C
Right this in increasing order of Ionization Energy: N,O,C
C, N, O
How do electronegativites increase?
Electronegativities generally increase from left to right across a period. This is due to an increase in nuclear charge. Alkali metals have the lowest electronegativities, while halogenshave the highest. Electronegativities generally decrease from top to bottom within a group due to the larger atomic size.
Shells
Energy levels where the electrons are found, the outer level is farther away, so attractive force of nucleus is smaller
What element has the lowest ionization energy? Highest?
Fr, F
Explain why the trends for ionization energy and electronegativity are the same.
If you have a high electronegativity then you have a really good job at attracting electrons, but it would take a really high ionization level to take an electron away
Which of the following elements will have a larger ionization energy: Magnesium (Mg) or calcium (Ca)? Why?
Magnesium has larger ionization energy than Calcium because Calcium is a larger atom, meaning that electrons are not easily pulled off from the atom (because they are closer to the positive attraction).
Which element will have a larger electronegativity: Magnesium or strontium? Why?
Magnesium will have a lower electronegativity than strontium because strontium is further down on the Periodic table, and has a large atomic size.
Electronegativity-Increasing- Co or P
P
Ionization-Increasing- Si or Fe
Si
Which of the following reasons explains why sulfur (S) will have a larger ionization energy than aluminum (Al)?
Sulfur has more protons in its nucleus and thus, holds its electrons more tightly.
Why does electronegativity decrease top to bottom?
This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus
Why does electronegativity increase left to right?
This occurs due to a greater charge on the nucleus, Fluorine is the most electronegative element.
Electronegativity-Increasing- K or Ti
Ti
How about Reactive Metals, will they have a high or low inaction energy?
Why do metals have a low ionization energy? Because the valence electrons are farther away from the positively charge nucleus, so the force of attraction is low
What is electronegativity?
ability of an atom to attract electrons
What is electronegativity?
ability of an atom to attract electrons when bonding with other elements
Within a group, the ionization energy decreases
as the size of the atom gets larger.
The highest electronegativity value
is for fluorine.
How does ionization energy increase?
left to right, bottom to top
What is electron Shielding?
loosens attraction between the nucleus and the farthest away electrons MAKES IT EASIER TO LOOSE A VALANCE ELECTRON
Explain why ionization energy decreases as you move down a group
one progresses down a group on the periodic table, the ionization energy will likely decrease since the valence electrons are farther away from the nucleus and experience greater shielding. They experience a weaker attraction to the positive charge of the nucleus.
increases. We can explain this by considering the nuclear charge of the atom. The more protonsin the nucleus,
the stronger the attraction of the nucleus to electrons. This stronger attraction makes it more difficult to remove electrons.
Why does electronegativity decrease down a group?
the valence electron is farther from the nucleus and harder to attract
For any given atom, the outermost valence electrons
will have lower ionization energies than the inner-shell kernel electrons. As more electrons are added the outer electrons become shielded from the nucleus by the inner shell electrons. This is called electron shielding.
