Quiz 7 Warner

How many valence electrons do alkali metals have?

1

Which element would you expect to have the lowest first ionization energy in this part of the periodic table?

Al

Which of the following is the correct order of increasing size of atomic radii?

Al<Ga<In

_________ earth metals are elements in group 2 of the periodic table.

Alkaline

Which of the following has the largest atomic radius?

B

The largest atom in the sixth period is _____.

Cesium

P, Al, Cl, Si, Na, S, Mg Which of the elements above is the most electronegative?

Cl

Which of the following has the smallest atomic radius?

F

Which of the following elements has the lowest ionization energy?

K

The table above represents part of the second period of the periodic table, with each element placed below its atomic number. Which element out of these is the least electronegative?

Li

A more stable electronic configuration shows:

More ionization energy will be required to remove an electron

Among the following, which element of the third period has the largest atomic radius?

Na

____ _____are nonreactive, nonmetallic elements in group 18 of the periodic table.

Noble gases

Arrange the following atoms in order of decreasing atomic radius:

Rb, Sr, Sn, Ge, P

_____ has the largest atomic radius.

Rubidium

Out of Sb, Bi, Md and Tm, _____ has the smallest atomic size and _____ has the largest atomic size.

Sb, Md

Which of the following elements has the lowest electronegativity value?

Si

Arrange the following atoms in order of decreasing atomic radius: Ga, As, Sn, Sb, Te

Sn, Sb, Te, Ga, As

Which of the following explains why ionization energy decreases down a group?

The atomic radius increases, so electrons are farther from the nucleus

Which of the following is true?

The electronegativity of calcium is lower than gallium

In the periodic table, the element with the largest atomic radii is found in:

The lower left

Which electron is the first to be removed from any atom?

a valence electron

Which alkaline earth metal is used as a contrast agent for x-rays of the digestive tract?

barium

The Pauling scale of electronegativity was based on:

bond energy

Which halogen is a dark orange liquid?

bromine

Atomic size increases across a period.

false

Nonmetals have low electronegativity value.

false

Nuclear charge decreases as the atomic number increases.

false

The atomic radius of carbon is 140 pm.

false

The atomic radius of lithium is smaller than beryllium.

false

With an increase in the nuclear charge, the force of attraction between the nucleus and the outer-most electrons decreases.

false

Nitrogen has a lower ionization energy value than _____ when moving from beryllium to neon.

fluorine

Noble gases are almost completely _______ because they have eight valence electrons.

nonreactive

If "n" stands for a given principal energy level, what is the outer electron configuration of the alkaline earth metals?

ns2

If "n" stands for a given principal energy level, what is the outer electron configuration of the halogens?

ns2np5

Cesium has a greater atomic radius than lithium.

true

The effective nuclear charge and the atomic size help explain the trend of ionization energy of atoms in a periodic table.

true

The picometer is the unit used to measure atomic radii.

true

Which statement(s) are TRUE about noble gas compounds?

- Only helium and neon have not formed compounds. - Only larger noble gases can form compounds.

The difference between the second and the third ionization energies of oxygen is _____.

1,910 kJ/mol

What will be the atomic radius of copper, if the distance between two adjacent copper atoms in metallic copper is 256 pm?

128 pm

The atomic radius of a nitrogen atom is 70 pm. What is the distance between the nuclei of two bonded nitrogen atoms in a N2N2 molecule?

140 pm

Which of the following is the electron configuration for a lithium atom?

1s2 2s1

The approximate electronegativity value of the most electronegative element on the Pauling scale is _____.

4

How many valence electrons do all halogens have?

7

Which of the following is the atomic radius of chlorine if the internuclear distance between two chlorine atoms is 198 pm?

99 pm

Elements A, B and C have following relations. B is in the same group as A and B's period number is larger than A's. C is in the same period as B and C's atomic number is less than B's. The relation of their atomic radii is:

A < B < C

When an element of very low ionization potential is allowed to react with an element of very high electron affinity, _____ is obtained.

A strong ionic bond

Element A is a good conductor of heat and electricity. A has strong reducibility and can form compounds with O only by 1:1. A is:

Alkaline earth metal

Element A is metallic and locates in the Group 1 on the periodic table. Element B has one more electron than A. B is a(n)

Alkaline earth metal

Which of the following is not an alkali metal?

Aluminum

How are most ions formed?

An atom transfers electrons to or from another atom or molecule.

Which of the following orders these elements by increasing ionization energy?

Ba, Ca, As, P, Cl

Which element has the greatest first ionization energy in this part of the periodic table?

Be

Which member of the alkaline earth metals has the highest electronegativity?

Be

The atomic radius of aluminum is greater than _____.

Boron

Which of the following is larger in atomic size?

Boron

Arrange the following atoms in order of the diagram of atomic radius above:

Br, Ge, Sn, Sr

Which of the following elements has the largest atomic radius?

Ca

Atomic radius ___ across a period.

Decreases

In the periodic table, moving right from tantalum (Ta) to mercury (Hg), the atomic radii:

Decreases

Which diagram shows the relation between the atomic numbers (Z) and the atomic radius (r) of elements in the same period?

Diagonal straight line going down

The attraction that an atom exerts on a pair of electrons which are being shared with another atom for the formation of covalent bonds is referred to as its _____.

Electronegativity

When _____ is measured on the Pauling scale, it gives a quantity which is/has _____.

Electronegativity, dimensionless

The table above represents a small piece of the periodic table with each element represented by it's symbol and atomic number. Which element here has the greatest electronegativity?

F

Which member of the halogen elements has the highest electronegativity?

F

Which ionization energy of the following has the greatest value?

First ionization energy (Si → Si+)

The covalent radius of bromine is:

Half the Br-Br bond length

Which group/family contains elements with the smallest radius within the same period?

Halogens

What happens to an atom when it gains electrons?

It becomes a negatively charged ion.

What happens to an atom when it loses electrons?

It becomes a positively charged ion.

Which member of the alkali metals has the highest electronegativity?

Li

Which of the following elements has the largest ionization energy?

Li

Considering the second period elements, which of the following has the largest atomic radius?

Lithium

The _____ electronegativity of metals and _____ electronegativity of non-metals means the reaction is most favorable between a metal and a non-metal.

Low, High

Which of the following has the largest atomic radius?

Na

A is an alkaline earth metal. If A loses two electrons to gain a complete octet, it has the same number of electrons as a(n)

Noble gas

Which statement best explains the reactivity of noble gases?

Noble gases are typically unreactive since they have full outer electron shells.

In general, as an approximation, elements with an electronegativity value of 2.0 or greater are _____.

Nonmetals

Which of the following elements will have the highest electronegativity?

O

Which list of elements from Period 2 is arranged from highest to lowest ionization energy?

O, N, B

The atomic size of silicon is greater than _____.

Phosphorus

Which of the following has the largest atomic radius among Group 16 elements?

Po

Electronegativity decreases from top to bottom within a respective group as:

Proceeding down the group, the size of atoms increases so the effective nuclear charge decreases on the electrons

Which of the following best explains why atomic radius decreases left to right across a period?

Protons are added to the nucleus, and the force of attraction on electrons is stronger

Which member of the alkaline earth metals has the smallest electronegativity?

Ra

Which of the following is the correct order of the increasing size of atomic radii?

Si<Sn<Pb

The atomic radii of oxygen and fluorine are _____ nitrogen.

Smaller than

When moving from left to right across a period,the outer electrons feel a _____ attraction towards the nucleus and the atomic radius _____.

Stronger, decreases

Why is atomic radius not a well-defined quantity?

The boundary of an electron cloud is not distinct.

Which of the following explains why electronegativity decreases from right to left across a period?

The number of protons decreases, so the nucleus is less positively charged

How does the principal energy level and the nuclear charge of an atom change in going from left to right across a period?

The principal energy level stays the same and the nuclear charge increases.

If two bonded atoms have the same electronegativity:

The shared pair of electrons will lie exactly in the center

During most chemical reactions, what happens to the atoms of a halogen?

They gain one electron.

Which group has the lowest electronegativities?

alkali metals

Which of following has the lowest value of ionization energy?

alkali metals

Which other elements of the periodic table do halogens readily react with to form halide salts?

alkali metals and alkaline earth metals

Ionization energy depends upon:

all of the above

Which of the following is/are true?

all of the above

Which element has a larger atomic radius than phosphorus?

aluminum

Negatively charged ions are called _____.

anion

Where are halogens frequently found in nature?

as salts in the ocean

Which alkaline earth metal is used as a white pigment in paints and toothpaste?

calcium

Positively charged ions are called _____.

cation

Atomic radii _____ while moving from scandium to chromium.

decrease

Atomic radius generally _____ from left to right across a period of the periodic table.

decreases

Ionization energy generally _____ from top to bottom down a group of the periodic table.

decreases

When moving from the third period to the seventh period, ionization value _____.

decreases

horizontal diagram In the diagram of elements above, which of the following describes the change of atomic radius along the direction of the arrow?

decreases

The reactivity of a given element is most closely related to its _____.

electron configuration

Among halogens, chlorine is the most electronegative element.

false

An effective nuclear charge is the charge actually felt by the outer electrons and is more than the actual nuclear charge.

false

An ion always has the same number of protons and electrons.

false

As the size of an atom increases, the energy required to remove the outermost electron also increases.

false

Atomic radii in transition metals follow a systematic order while moving from left to right.

false

Atomic radii increase in size with an increase in the atomic number across a period.

false

Electron affinity and electronegativity are both measured in energy units.

false

Electronegativity generally increases while moving from top to bottom in the periodic table.

false

Electronegativity increases as you move from aluminum to thallium down the group 13 elements.

false

Electronegativity is directly related to the metallic properties of elements.

false

Group 1A elements have two electrons in their outer shell.

false

Hydrogen is considered to be an alkali metal.

false

Ionization energy is expressed in the units of electron volts per atom.

false

Ions form because the loss of one or more electrons makes them less stable than their corresponding atoms; this state requires more energy to maintain.

false

The atomic radius tends to increase as progression is made across a period from left to right.

false

The atomic size of beryllium is larger than lithium.

false

The attraction between the nucleus and electrons increases while moving down a group in the periodic table.

false

The electronegativity value is lowest in polonium when we move from left to right in the sixth period.

false

The first ionization energy of hydrogen is greater than that of helium.

false

The first ionization energy of rubidium is higher than that of sodium.

false

The first ionization energy of silicon is less than the first ionization energy of aluminum.

false

The force of attraction between the nucleus and an electron decreases with an increase in nuclear charge.

false

The ionization energy generally increases down the group.

false

The larger the value of ionization energy, the easier it is to remove an electron from an atom.

false

The number of valence electrons present in alkali metals are 2.

false

The outer electrons shield the inner electrons from the positive charge of the nucleus.

false

The shielding effect makes it easier to remove the outer most electrons from those atoms which have many electrons. Therefore ionization energy will increase while moving down a group.

false

The size of an atom is independent of the number of protons in the nucleus, the number of energy levels holding electrons, and the number of electrons in the outer energy level.

false

There is no difference between electron affinity and electronegativity.

false

True or False: Among all halogens, fluorine has the smallest electronegativity

false

True or False: At room temperature and 1 atm, all gases are diatomic molecules.

false

True or False: Atomic radius increases down a group because the the number ofvalence electrons increase with increasing electrons.

false

True or False: Cl, Pb, Sn, Ar, Se, Br The order of increasing atomic radius of all atoms above is:

false

True or False: In Group 16, S has the smallest atomic radius.

false

True or False: Ionization energy increases down a group because the number of protons increases and it's more difficult to lose electrons.

false

When a graph is plotted between atomic radii versus the number of protons for the first transition metal series, a straight line is formed.

false

When moving from antimony to iodine, the first ionization energy value decreases.

false

When moving from gold to lead, the atomic radius increases.

false

When we move from boron to carbon, atomic size increases.

false

While moving across the periodic table from left to right there is an increase in atomic radius. .

false

While moving from aluminum to thallium, gallium has an electronegativity value lower than indium.

false

Arrow directions represent increasing trend of ionization energy. Which of the following correctly shows the general trend?

first arrow is vertical going up and second is horizontal going right

The element _____ is assigned the highest electronegativity, with a value of ____.

fluorine; 4.0

Which diagram shows the relation between the atomic numbers (Z) and the atomic radius (r) of elements in the same group?

graph with diagonal straight line going up

The first ionization energy of sodium is _____ than potassium.

greater

Compared to the ionization energy of a lithium atom, the ionization energy of a beryllium atom is larger. This is primarily a result of the beryllium atom having:

greater nuclear charge

Where are the alkali metals located in the periodic table?

group 1

Halogens are located in what group on the periodic table?

group 17

Alkaline earth metals are located in what group on the periodic table?

group 2

Where are the alkaline earth metals located in the periodic table?

group 2

Element A is located between group 16 and noble gas on the periodic table. A is a(n)

halogen

Which group has the highest electronegativities?

halogens

Across a period, the effective nuclear charge increases and therefore it becomes _____ to remove an electron.

harder

In the following elements, _____ has the highest ionization energy.

helium

As the number of valence electrons increases, the electronegativity value becomes _____.

higher

What gas is produced when an alkali metal reacts with water?

hydrogen only

Ionization energy generally _____ from left to right across a period of the periodic table.

increases

The electronegativity value _____ when one moves from beryllium to nitrogen.

increases

Upon moving down in a group, the distance between the valence electrons and the nucleus _____.

increases

When moving down a group,the atomic size _____ and therefore the ionization energy decreases.

increases

vertical diagram In the diagram of elements above, which of the following describes the change of atomic radius along the direction of the arrow?

increases

Which halogen is a purple-gray solid?

iodine

Which of the following halogens has the largest atomic radius?

iodine

If an atom gains or loses electrons, it becomes a(n) _____.

ion

Compared to the ionization energy of a magnesium atom, the ionization energy of a calcium atom is smaller. This is primarily because the calcium atom:

is larger than the magnesium atom

Compared with alkali metals, the alkaline earth metal in the same period has ___ electronegativity.

larger

In alkali metals, the atomic radius of potassium is greater than _____.

lithium

What would be the name for Li+?

lithium ion

When a group 1 element reacts it

loses one electron.

Metals tend to have generally _____ electronegativities, while nonmetals tend to have generally _____ electronegativities.

low; high

Elements in the alkaline earth metal family of the periodic table have ________ electronegativity values than elements in the halogen family of the periodic table.

lower

Which alkaline earth metal is found in flares?

magnesium

P, F, Cl, Si, C, O, Mg Which of the elements above is the least electronegative?

mg

The second ionization energy is greater than the first because it's ___ to remove an electron from a cation.

more difficult

Which of the following has the highest ionization energy?

neon

Which of the following characteristics of halogens is not correct?

none of the above

If "n" stands for a given principal energy level, what is the outer electron configuration of the noble gases (except He)?

ns2np6

The ______ rule is based on the number of electrons in the noble gases, which are the least reactive elements.

octet

_________ proposed the first scale of electronegativity.

pauling

Complete the sentence using one of the following terms: s, p, d, or f. Alkali metals are a part of the ____ block of the periodic table.

s

Complete the sentence using one of the following terms: s, p, d, or f. Alkaline earth metals are a part of the ____ block of the periodic table.

s

The presence of inner-shell electrons cause the outermost electrons of an atom to be less attracted to the nucleus. This is called electron _____.

shielding

_____ has the smallest atomic radius.

silicon

Compared with halogens, the alkali metal in the same period has ___ electronegativity.

smaller

Which of the following elements has the lowest ionization energy?

sodium

Which of the following is not a Group 2A element?

sodium

Which alkaline earth metal is used in red fireworks?

strontium

Which element has the highest first ionization energy?

sulfur

Compared to the atomic radius of a carbon atom, the atomic radius of a silicon atom is larger because of an increase in:

the number of principal energy levels

An effective nuclear charge is the charge experienced by a specific electron within an atom.

true

An increase in the number of electrons in an atom will result in a decrease in the ionization energy.

true

Atomic radii decrease while moving left to right across the periodic table.

true

By having knowledge of the atomic radius of an atom, the size of the atom can be measured.

true

Cesium is considered the most electropositive stable element.

true

Cesium is the most electropositive stable element of all the alkali metals.

true

Chlorine has a larger atomic radius than fluorine.

true

Group 1A elements are highly reactive.

true

Group 2A elements are moderately hard.

true

In the second period, the atomic radii decrease as one moves from lithium to neon.

true

Metalloids have electronegativity values close to 2 (on the Pauling scale).

true

Moving across a period from left to right increases the ionization energy.

true

Non-metallic elements have high electronegativity.

true

The ability of an atom in a molecule to attract shared electrons is called electronegativity.

true

The alkali metals, which are at the extreme left of the periodic table, have the largest size in the periodic table.

true

The atomic radius of xenon is greater than helium.

true

The atomic size is the distance from the nucleus to its outermost shell of electrons.

true

The attractive force between the outer-most electrons and the nucleus of an atom is inversely proportional to the distance between them.

true

The elements of Group 1A have the largest atomic radii in their periods.

true

The first ionization energy values of Zn, Cd, and Hg are relatively higher than their immediate neighbors.

true

The size of atomic radii within a group of elements increase while moving from top to bottom.

true

The tendency of an atom to attract the shared pair of electrons towards itself in a covalent bond is known as electronegativity.

true

True or False: A is a metal in the same group as Na, so A is an alkali metal.

true

True or False: Astatine is located in group 17 so it is considered a halogen element.

true

True or False: Cesium is an alkali metal.

true

True or False: Ionization energy increases across a period, because it's more difficult to lose electrons as the number of protons increase.

true

Ways in which ions may form include ______.

two of the above

Which describes the state that the noble gases are found at room temperature?

unreactive monatomic gases

Chemical bonds involve the transfer or sharing of _____.

valence electrons only

With which noble gas was the first noble gas compound finally formed?

xenon