periodic trends
which electron configuration represents a transition element
(Ar)3d54s2
what trend in atomic radius do you see as you go down a group/family on the periodic table?
-as u go down, ionization energy decreases. -#of energy levels increase as you go down
As the elements of group 1 on the periodic table are considered in order of increasing atomic radius the ionization energy of each successive element generally
decreases
which of these elements has the least attraction for electrons in a chemical bond
nitrogen
which group tends to form -1 ions?
noble gases
what is the total number of valences electrons in an atom of boron in the ground state
3
what is the total number of valence electrons in an atom of xenon, Xe?
8
what causes this trend?
Adding more energy
which element in period 5 of the periodic table is a transition element
Ag
which sequence of elements is arranged in order of decreasing atomic radii
Al,Si,P
which element out of Au, Zn, S, and Si has the largest atom?
Au
which element out of Au, Zn, S, and Si has the most metallic character?
Au
which of the following group 2 elements has the lowest first ionization energy
Ba
which list of elements from group2 on the periodic table is arranged in order of increasing atomic radius
Be,Mg,Ca
which element out of P,S,Cl, and F has the highest electronegativity ?
F
which element out of P,S,Cl, and F has the least metallic character?
F
which group tends to form +1 ions
Group 1
Which Group 17 element has the least attraction for electrons?
I
which element is a member of the halogen family
I
which sequence correctly places the elements in order of increasing ionization energy?
I-Br-CI-F
which of the following atoms has the largest atomic radius
K
which element out of Li, Be, Mg, and Na is the largest atom?
Mg
What causes this trend?
More protons, more pull.
which element out of Li, Be, Mg, and Na has the least metallic character?
Na
which element out of Li, Be, Mg, and Na has the lowest electronegativity ?
Na
Which element in Group 16 has the greatest tendency to gain electrons?
O
put the following in order from smallest to largest atomic radius C,O,Sn,Sr
O,C,Sn,Sr
which element out of P,S,Cl, and F has the largest ion?
P
which element out of Au, Zn, S, and Si has the highest electronegativity?
S
Define electronegativity
a chemical property that describes the ability of an atom to attract electrons towards itself
an element with a partially filled d sub level in the ground state is classified as
a transition metal
What trend in electronegativity do you see as you go across a group/family on the periodic table?
electronegativity decreases as you move left to right across a periodic table
What trend in electronegativity do you see as you go down a group/family on the periodic table?
electronegativity of an element increases because the increased number of energy levels puts the outer electrons very far away from the pull of nucleus.
the strength of an atoms attraction for the electrons in a chemical bond is the atoms
electronnegativity
the amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as
first ionization energy
the group 17 element with the highest electronegativity is
fluorine
which group tends to form +2 ions
group 2
Which noble gas has the highest first ionization energy?
helium
which properties are most common in nonmetals
high ionization energy and high electronegativity
As each successive element in Group 15 of the Periodic Table is considered in order of increasing atomic number, the atomic radius
increases
the ability of carbon to attract electrons is
less than that of nitrogen and oxygen
the elements calcium and strontium have similar chemical properties beacasue they both have the same
number of valence electrons
what causes this trend
organization of elements
how does the ionic radius of a nonmetal compare with its atomic radius?
the ionic radius of a nonmetal is larger than its neutral atom
What trend in atomic radius do you see as you go across a period/row on the periodic table?
the ionization energy increases because the # of protons increases as you go across.
which statement best describes group two elements as they are considered in order from top to bottom of the periodic table
the number of principal energy levels increases, and the number of valence electrons remains the same.
As the elements Li to F in Period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the covalent radius of each successive element compare?
the relative electronegativity increases and the atomic radius decreases
on the periodic table of the elements all the elements within group 16 have the same number of
valence electrons
