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What is the general trend in ionization energies of elements in the same chemical family?
Mcsidney123
Chemical families are also known as the columns on the periodic tables.
The general trend is that the amount of energy required to lose an electron decreases as you move down a column, or chemical family.
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∙ 12y ago
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What are the general properties of the elements in the group on the right side of the periodic table?
The elements present at right side groups of the periodic table are non-metals. They have high electron affinity and ionization energy.
What is the relationship between elements and the periodic table and ionisation energy?
The relationship between atomic numbers and first ionization energies is that within the same period, as atomic number increases so does first ionization because as nuclear charge increases and atomic radius decreases, electrons become harder to remove. However, within the same group, the first ionization energy decreases as atomic number increases because of the added energy level, the electrons are farther from the nucleus and easier to remove.
What are the general and characteristics of metals and non metals and metalloids?
Metals: Shiny 'metallic' appearance Solids at room temperature (except mercury) High melting points High densities Large atomic radii Non Metals: High ionization energies High electronegativities Poor thermal conductors Poor electrical conductors Brittle solids Little or no metallic luster Gain electrons easily Metalloids: Electronegativities between those of metals and nonmetals Ionization energies between those of metals and nonmetals Possess some characteristics of metals/some of nonmetals Reactivity depends on properties of other elements in reaction Often make good semiconductors
What is the second ionization of energy and how does it work?
Imagine that one electron has already been removed from an atom, the energy used to accomplish this is the 1st ionization energy. Now more energy is needed to remove a 2nd electron. That is the 2nd ionization energy.
How would you descibe the arrangement of the periodic table?
The two main arrangements of the periodic table are the groups, which form the columns of the table, and the periods, which form the rows. There are some similarities between elements in the same period, but most similarities are shared within the groups of elements.
Is the pattern in ionization energy always true or generally true?
there is always a decrease in ionization energies down a group, and there is always a general increase across each period. this is always true.
Which statement describes the general trends in electronegativity and first ionization energy as the elements in Period 3 are considered in order from Na to Cl?
The Pauling electronegativity and the first ionization energy increase from sodium to chlorine.
Which has a greater ionization energy beryllium or germanium?
Beryllium has greater ionization energy, with 899 kJ/mol versus Germanium's 762 kJ/mol. The general trend (most prominently displayed in the representative elements) in the periodic table is increasing ionization energy across a period, and decreasing ionization energy down a group.
Why do non metals have higher ionization energies than metal?
Ionization energy is the energy needed to remove an electron. Elements other than transition metals gain or lose electrons from the s and p orbitals in order gain the more stable electron configuration of a Noble gas. Metals lose electrons to become isoelectronic (that is have the same electron configuration) to a noble gas (previous to them in the periodic table), while nonmetals tend to gain electrons in order to become isoelectronic to a Noble gas (next highest on the periodic table). Since ionization energy is the energy needed to REMOVE an electron, it is low for metals which form positive ions by losing electrons to become more stable, but very high for nonmetals that tend to gain, NOT LOSE, electrons. Most transition metals tend to lose electrons as well (other than Rhenium). Transition metals lose electrons from the d orbital, but still form positive ions, so their ionization energy is also usually lower than nonmetals.
What trend is seen on the periodic table?
"Electronegativity"
What are the general properties of the elements in the group on the right side of the periodic table?
The elements present at right side groups of the periodic table are non-metals. They have high electron affinity and ionization energy.
What is the relationship between elements and the periodic table and ionisation energy?
The relationship between atomic numbers and first ionization energies is that within the same period, as atomic number increases so does first ionization because as nuclear charge increases and atomic radius decreases, electrons become harder to remove. However, within the same group, the first ionization energy decreases as atomic number increases because of the added energy level, the electrons are farther from the nucleus and easier to remove.
What are the elements or compounds that are produced by a chemical reaction?
The general term is "products", intuitively enough.
What is the general trend of ionization energy as you go across the periodic table?
Across a period, first ionization energy increases. However, when going down a group, first ionization energy generally decreases. As you go down a group, atoms hove more total electrons so they don't really care that much about their outermost ones.
What are the general and characteristics of metals and non metals and metalloids?
Metals: Shiny 'metallic' appearance Solids at room temperature (except mercury) High melting points High densities Large atomic radii Non Metals: High ionization energies High electronegativities Poor thermal conductors Poor electrical conductors Brittle solids Little or no metallic luster Gain electrons easily Metalloids: Electronegativities between those of metals and nonmetals Ionization energies between those of metals and nonmetals Possess some characteristics of metals/some of nonmetals Reactivity depends on properties of other elements in reaction Often make good semiconductors
What accounts for the general trend in the first ionuization energy of the elements within a period?
As you go from right to left in a period in the periodic table the ionization energy increases. While going from top to bottom in a group in the periodic table the ionization energy decreases .
What is the second ionization of energy and how does it work?
Imagine that one electron has already been removed from an atom, the energy used to accomplish this is the 1st ionization energy. Now more energy is needed to remove a 2nd electron. That is the 2nd ionization energy.
