periodic trends

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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


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