Periodic Trends Review

Which of the following elements has the smallest ionization energy? Ca, O, S, K

Ca

Arrange the following elements in order of increasing electronegativity: calcium, selenium, arsenic

Calcium, arsenic, selenium

Which element has a larger electronegativity, Silicon or Chlorine?

Chlorine

Which elements reacts most vigorously with water to produce hydrogen gas? Li, K, P, Cs

Cs

Atomic radius of F, Br, and I is 64, 114, and 138 pm; estimate a reasonable atomic radius of Cl: 53 pm, 89 pm, 126 pm, 162 pm

89 pm

Electronegativity tends to increase as you A) go down a column of the periodic table B) go from left to right across the periodic table C) Go toward the middle of the periodic table D) going from top right to bottom left of periodic table

B

Will the electronegativity of barium be larger or smaller than that of strontium? Explain by drawing Bohr models

Ba is larger in size (it has an extra energy level when you draw it), so it has a larger atomic radius; the force of attraction goes down when distance increases, so Ba is not as strong at attracting electrons as Sr; therefore, Ba has smaller electronegativity

Which element has a smaller ionization energy, Xenon or Barium?

Barium

What has the larger atomic radius, Boron or Fluorine?

Boron

Compare and contrast ionization energy and electronegativity; In general, what can you say about these values for metals and non-metals?

Both ionization energy and electronegativity increase as you go up and to the right; metals have low ionization energy and electronegativity; non-metals have high ionization energy and electronegativity

In your own words, define electronegativity and the general trend of electronegativity in the periodic table

Electronegativity is the ability of atoms to pull in electrons; the trend = it is the lowest in the bottom left and increases towards the upper right

Use the periodic table to predict which element has the largest ionization energy; H, F, Fr, Rn

F

Why does fluorine have a higher ionization energy than iodine?

Fluorine is smaller and has a stronger force of attraction; therefore it requires more energy to take away its electrons

Use the periodic table to predict which element has the largest atomic radius: H, He, Fr, Rn

Fr

Highly reactive, especially with alkali metals and alkaline earths; most reactive nonmetals

Halogens

Which of the following elements has the smallest atomic radius: He, Bi, O, F

He

In your own words, define ionization energy and the general trend of ionization energy in the periodic table

Ionization energy is the energy needed to take away an electron from an atom; the trend = it is the lowest in the bottom left and increases toward the upper right

Which of the following elements has the greatest electronegativity? Li, K, Na, Fr

Li

Which of the following elements has the greatest electronegativity? Li, Be, N, C

N

Which of the following elements has the largest atomic radius? Ne, F, O, N

N

Germanium is used in the manufacturing of some transistors; what other element is similar?

Si

Which of the following elements has the least electronegativity? Sr, Ca, O, S

Sr

Compare the electronegativity of tellurium to that of antimony; Explain your reasoning using Bohr models

When you draw Sb and Te, they appear to be the same size; however, Te has one more proton than Sb, so it will have a stronger force of attraction for electrons than Sb; Te will therefore have a greater electronegativity; also, the electron shells of Te will be "pulled in" more than Sb because of this stronger attraction

any of the elements beryllium, magnesium, calcium, strontium, barium, and radium, occupying Group IIA (2) of the periodic table

They are reactive, electropositive, divalent metals, and form basic oxides that react with water to form comparatively insoluble hydroxides.alkaline earth metals

any of the set of metallic elements occupying a central block (Groups IVB-VIII, IB, and IIB, or 4-12) in the periodic table, ex: iron, manganese, chromium, and copper; chemically they show variable valence and a strong tendency to form coordination compounds, and many of their compounds are colored

Transition metals

they are good conductors of heat and electricity

Transition metals

they are less reactive than alkali metals such as sodium

Transition metals

they can be hammered or bent into shape easily

Transition metals

they form coloured compounds

Transition metals

they have high melting points - but mercury is a liquid at room temperature

Transition metals

Electronegativity

a measure of the ability of an atom's nucleus to attract electrons from a different atom within a covalent bond

any of the elements lithium, sodium, potassium, rubidium, cesium, and francium, occupying Group IA (1) of the periodic table;They are very reactive, electropositive, monovalent metals forming strongly alkaline hydroxides

alkali metals

Relationship between electronegativity and atomic number in a period

as one increases, the other increases

What is the trend for atomic radius going across the period from left to right?

it decreases

What is the trend for ionization energy from left to right?

it increases

The ability of an atom to attract electrons is called the

electronegativity; electron affinity

For which of the properties does Lithium have a larger value than Potassium? Neutrons, atomic radius, number of protons, first ionization energy

first ionization energy

Coulombic attraction is another way of saying

force of attraction between electrons and protons

Arrange the following elements in order of increasing electronegativity: phosphorus, oxygen, germanium

germanium, phosphorus, oxygen

Elements in the same column in the periodic table are referred to as being in the same

group; family

Because they are so reactive, elemental halogens are toxic and potentially lethal; Toxicity decreases with heavier halogens, until you get to astatine, which is dangerous because of its radioactivity

halogens

Highest electronegativities

halogens

Seven valence electrons (one short of a stable octet)

halogens

The group within any period with the greatest electronegativity is usually the ___

halogens; Halogens are the smallest elements in their period with the highest number of protons; they will have the strongest force of attraction; noble gases violate the trend as they are unreactive

What is the trend for electronegativity from bottom to top?

increases

Arrange the following elements in order of increasing electronegativity: gallium, aluminum, indium

indium, gallium, aluminum

Energy required to take away an electron from the outer energy level of an atom is called the

ionization energy

The more reactive element would have a (lower/higher) ionization energy

lower; the more energy you need to remove an electron, the harder it is to react

an element (ex: germanium or silicon) whose properties are intermediate between those of metals and solid nonmetals; are electrical semiconductors

metalloids

physical properties tend to be metallic, but their chemical properties tend to be non-metallic

metalloids

solid at room temperature

metalloids

Good conductors of heat and electricity

metals

Hard

metals

High density (are heavy for their size)

metals

High melting and boiling points

metals

High tensile strength (resist being stretched)

metals

Lustrous (shiny)

metals

Malleable (can be beaten into sheets)

metals

Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, Aluminum

neon, aluminum, sulfur, oxygen

Which of these elements has the least attraction for electrons in a chemical bond? Oxygen, nitrogen, fluorine, chlorine

nitrogen

This group has the highest ionization energy levels and the lowest electronegativity levels

noble gases

odorless, colorless, monatomic gases with very low chemical reactivity

noble gases

Brittle solids - not malleable or ductile

nonmetals

Dull, not metallic-shiny, although they may be colorful

nonmetals

Gain electrons easily

nonmetals

High electronegativities

nonmetals

High ionization energies

nonmetals

Little or no metallic luster

nonmetals

Poor electrical conductors

nonmetals

Poor thermal conductors

nonmetals

Elements in the periodic table are grouped by their

number of outside/valence electrons

Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, Potassium

oxygen, carbon, aluminum, potassium

Elements in the same row of the periodic table are referred to as a

period

Metametals; The metametals are zinc, cadmium, mercury, indium, thallium, tin and lead; They are ductile elements but, compared to their metallic periodic table neighbours to the left, have lower melting points, relatively low electrical and thermal conductivities, and show distortions from close-packed forms

post-transition metals

Arrange the following elements in order of increasing electronegativity: oxygen, fluorine, sulfur

sulfur, oxygen, fluorine

Ionization energy

the amount of energy needed to remove an electron from an atom

Which statement 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

Why do elements in the same group generally have similar properties?

they have the same number of valence electrons so they react similarly

Which of the following is a transition element? Sodium, Chlorine, titanium, aluminum

titanium

groups 3-12 in the periodic table, are generally characterized by partially filled d subshells in the free elements or their cations

transition metals