chem chapter 6

what is the total number of valence electrons in the Atom of boron in the ground state

3

what is the total number of valence electrons in an Atom of xenon

8

compared to the atomic radius of a sodium atom The atomic radius of a magnesium atom is smaller the smaller radius is primarily a result of the magnesium atom having

A larger nuclear charge

each. In the periodic table corresponds to

A principal energy level

which element in period Five of the periodic table is a transition element: Sr, sb, ag, xe

Ag

which sequence of elements is arranged in order of decreasing atomic radii: al, si, p. li, na, k. cl, br, I. n, c, b.

Al, Si, P.

which of the following group 2 elements has the lowest first ionization energy: be, mg, ca, ba

Ba

which lists of elements from group to on the periodic table is arranged in order of increasing atomic radiius: be, mg, ca. ca, mg, be. ba, ra, Sr, sr, ra, ba.

Be, Mg, Ca

Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements

Dmitri mendeleev

which element is a member of the halogen family: k. b. I. s.

I

which group 17 element has the least attraction for electrons: f. cl. br. I.

I

which sequence correctly places the elements in order of increasing ionization energy: h, li, na, k. I, br, cl, f. o, s, se, te. h be, al, ga.

I, Br, Cl, F

which of the following Adams has the largest atomic radius: Na. k. mg. ca.

K

of the elements pt, v, li, and kr, which is a nonmetal

Kr

which of the following elements has the smallest ionic radius: li, k, o, s

Li

The modern periodic table is arranged in order of increasing atomic

Number

The elements calcium and strontium have similar chemical properties because they both have the same

Number of valence electrons

periodic law

States that the properties of elements show a periodic tendency when the elements are arranged in order of increasing atomic number

of the elements fe, hg, u, and te, which is a representative element

Te

nuclear charge

The amount of positive charge of an atom

The first electron removed from the atom is called

The first ionization energy

Coulomb's law

The force of attraction increases as the amount of charge increases or as the distance decreases between two oppositely charged objects (protons and electrons)

which of the following is true about the electron configuration of the noble gases: the highest occupied S and P sub levels are completely filled, the highest occupied s and p sublevels are partially filled, the electrons with the highest energy are in a D sub level, The electrons with the highest energy are in a F sub level

The highest occupied S and P sub levels are completely filled

The trends in properties of elements are related to

The nuclear attraction between the nucleus and valence electrons the number of electrons in and Atom is

what best describes group 2 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 and 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

effective nuclear charge

The screened attraction of the nuclear charge of an outer electron

what electron configuration represents a transition elements : 1s^2 2s^2 2p^5, [Ne] 3s^2, [Ar] 3d^5 4s^2, [Ar] 3d^10 4s^2 4p^6

[Ar]3d^5 4s^2

an element with the partially filled D sub level in the ground state is classified as

a transition metal

electronegativity

ability of an atom of a molecule to attract shared electrons to itself

of the following elements which one has the smallest first item ionization energy: boron, carbon, aluminum, silicon

aluminum

which of the following factors contributes to the increase in ionization energy from left to right across a period: An increase in the shielding effect, an increase in the size of the nucleus, an increase in the number of protons, fewer electrons in the highest occupied energy level

an increase in the number of protons

what is the element with the lowest electronegativity value: cesium, helium, calcium, fluorine

cesium

Ion

charged atom formed by the gain or loss of valence electrons from the neutral atom

ionic radius period Trend

decrease due to the increase of attraction between electrons and protons

atomic radii periodic trend

decrease due to the increasing attraction of protons and electrons

as the elements of group one on the periodic table are considered in order of increasing atomic radius the ionization energy of each successive element generally

decreases

ionization group trend

decreases because of the increase in shielding affect

electronegativity group Trend

decreases due to the increase of shielding affect

what subatomic particle plays the greatest part in determining the properties of an Atom

electron

The strength of an atoms attraction for the electrons in a chemical bond is the Atoms

electronegativity

which statement is true about electronegativity: electronegativity is the ability of an anion to attract another anion, electronegativity generally increases as you move from top to bottom with in a group, electronegativity generally is higher for metals than nonmetals, electronegativity generally increases from left to right across a period

electronegativity generally increases from left to right across a period

what causes the shielding affect to remain constant across a period

electrons are added to the same principal energy level

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 noble gas has the highest first ionization energy: radon. Krypton. Neon. Helium.

helium

what properties are most common in nonmetals

high ionization energy and high electronegativity

period trend in effective nuclear charge

increase because of increased nuclear charge

ionic radius group trend

increase due to the increase in energy levels

atomic radii group trend

increase increases energy levels

as each successive elements in group 15 of the periodic table is considered an order of increasing atomic number the atomic radius

increases

Ionization period trend

increases because of the increase in protons

electronegativity period Trend

increases due to an increase in protons

as elements of group one of the periodic table are considered in order from top to bottom the ionization energy of each successive element decreases this decrease is due to

increasing radius and increasing shielding effect

The amount of screening affected pens on the number of

inner core electrons

how does atomic radius change from top to bottom in a group in the periodic table

it tends to increase

The ability of carbon to attract electrons is

less than that of nitrogen and oxygen

what element in the second period Has the largest atomic radius: carbon, lithium, potassium, neon

lithium

which of the following elements is in the same period As phosphorus: carbon, magnesium, nitrogen, oxygen

magnesium

which of the following categories includes the majority of the elements: metalloids, liquids, metals, nonmetals

metals

which of these elements has the least attraction for electrons in a chemical bond: oxygen, fluorine, nitrogen, chlorine.

nitrogen

to what category of elements does an element belong if it is a poor conductor of electricity

nonmetals

which element in group 16 has the greatest tendency to gain electrons: te. se. s. o.

o

Group trend in effective nuclear charge

remains the same the number of energy levels between the nucleus and the valence electrons increase thus weakening The attraction of valence electrons of atoms

what element has electron configuration 1s^2 2s^2 2p^6 3s^2 3p^2: nitrogen, selenium,silicon, silver

silicon

ionization energy is required

to remove an electron from an Atom in the gaseous state

on the periodic table of the elements all the elements with an group 16 had the same number of

valence electrons

which of the following statements is true about ions: anions are positively charged ions, cations are common among nonmetals, charges for ions are always written as numbers followed by a plus or minus sign, when an anion forms more electrons are transferred to it

when an anion forms more electrons are transferred to it