Unit 6: Bonding With The Periodic Table Flashcards by Isabella DiLeo

How were elements originally arranged by in the periodic table? (Dimitri Mendeleev)

The original arrangement was based on ATOMIC MASS, and properties were used to sort the elements into groups.

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How are elements arranged in the modern periodic table? (Henry Mosley)

In the modern table, elements are arranged in order of INCREASING ATOMIC NUMBER.

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What are Groups on the periodic table?

Vertical columns that have the same # of valence electrons (with the exception of Helium, He), and similar chemical properties.

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What are Periods on the periodic table?

Horizontal rows that have electrons which fill in the same energy levels (EL).

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What are four important Group Names?

Alkali Metals [Group 1]
Alkaline Earth Metals [Group 2]
Halogens [Group 17]
Noble Gasses [Group 18]

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What are some Properties of [Group 1] Alkali Metals?

-Found in nature, only in compounds.
-Most ACTIVE METALS.
-Francium (Fr) is the MOST ACTIVE METAL.
-Form +1 ions (because they lose their one valence electron).

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What are some Properties of [Group 2] Alkaline Earth Metals?

-Found in nature, only in compounds.
- Reactive, but slightly less than Group 1.
-Form +2 ions (because they lose their 2 valence electrons).

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What are some Properties of [Group 17] Halogens?

-Found in nature, only in compounds.
-Most ACTIVE NON-METALS.
-Flourine (F) is the MOST ACTIVE NON-METAL.
-Form -1 ions (because they gain 1 valence electrons to obtain a full octet!)
-Only group where all elements exist in all 3 phases of matter at STP.

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What are some Properties of [Group 18] Noble Gasses.

[ALL ELEMENTS WANT TO BE LIKE THIS]
- Nonreactive and generally stable.
-Have a full octet (8 valence electrons).
*Except He (Follows the duet -> happy with 2 electrons)**

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What are some Properties of
[Groups 3-12] Transition Metals?

-Usually HIGH MELTING POINT METALS.
They have several possible ionic charges.
-They usually form colored compounds.
Ex.) Copper (Cu), Iron (Fe), Zinc (Zn).

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How are elements Divided on the periodic table?

-METALS [All elements to the LEFT of the bolded staircase].
-NON-METALS [All elements to the RIGHT of the bolded staircase].
-METALLOIDS [All Semi-metals (B, Si, GE, As, Sb, Te, At) that BORDER the bolded staircase].

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What are some Properties of Metals?

-Good conductors of heat and electric current.
-Solids at STP (except Hg).
-Ductile, Malleable, Luster (Shine).
-Most are a silvery-grey color (except copper and gold).

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What are some Properties of Non-Metals?

-Greater variation in physical properties.
-Many different states.
-Many different colors.
-Poor conductors of heat and electricity.
-Brittle.

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What is the activity of Metals and Non-Metals?

-Activity of metals INCREASES down a group. *The most active metal is Francium (Fr), which is located at the bottom left**
-Activity of Non-Metals decreased down a group. *The most active non-metal is Flourine (F), and it is located at the top right**

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What are some Properties of Metalloids/Semi-metals?

-They are located along the bolded staircase.
-They have properties of both Metals and Non-Metals.
-Their behavior is controlled by the environment.
Ex.) Silicon.

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What are some trends in Metallic properties?

-Metals want to lose electrons.
-Form positive (+) ions [Cations]
-Low Electronegativity.
-Low first ionization energy.
-Metallic properties decrease right across a period.
-Metallic properties increase down a group.
*The most metallic element is Francium (Fr) and it is the most active/reactive metal**

What are some trends in Non-Metallic Properties?

-Non-metals want to gain electrons.
-Form negative (-) ions [Anions]
-High electronegativity
-High first ionization energy.
-Non metallic properties increase right across a period.
-Non-Metallic properties decrease as you move down a group.
*The most non-metallic element is Flourine (F) and it is the most active/reactive non-metal**

How do you determine the phase of a substance based on its properties?

-If the melting point and boiling point are above STP [SOLID].
-If the melting point is below STP and the boiling point is above STP [Liquid].
-If the melting point and the boiling point are below STP [GAS].
*It takes LESS energy as heat to melt and boil**

What is the Periodic Law?

When elements are arranged in order of increasing atomic #, there is a periodic repetition of their physical and chemical properties.

What are Periodic Trends?

The succession of elements across the same period and down the same group that demonstrate characteristic periodic trends [Atomic radius, ionic radius, first ionization energy, electronegativity].

What is Atomic Radius?

Also called atomic size, it is defined as the distance between the center of the nucleus of an atom and the outermost electrons.

What is Atomic Size?

Atomic Size is the size of the atom that:
-INCREASES from top to bottom within a group.
-DECREASES from left to right across a period.

In a Group (From top to bottom):

-The atomic # increases.
-Nuclear Charge (# of protons) increases.
-An increase (+) in charge draws electrons closer to the nucleus. *Opposites Attract**
-# of occupied energy levels increases.
-An increase in the # of occupied orbitals “shells” shields electrons in the valence shell from the attraction of protons in the nucleus.

What is the Shielding Effect?

The shielding effect blocks the attraction of the nucleus for the outer electrons. It is greater than the effect of the increase in nuclear charge. *The atomic size INCREASES top to bottom down a group because the force of attraction is LESS**
STRONGER ATTRACTION WHEN CLOSER TO THE NUCLEUS (Smaller atomic size).
WEAKER ATTRACTION WHEN FARTHER AWAY (Larger atomic size).

Across a Period (Left to Right):

-Each element has 1 more proton and electron. -Electrons are added to the same principal energy level. -The shielding effect is constant for all elements in a period (same # of shells or orbitals). -The increasing nuclear charge pulls the electrons in the valence shell closer to the nucleus and the atomic size decreases.

What is the Oxidization Number?

A positive or negative number assigned to an atom to indicate its charge when combined into a compound. *The oxidization of an uncombined element is zero**

What are Metal Ions?

Atoms of metallic elements that tend to lose one or more electrons and form cations (+). -One less orbital and electrons are pulled in much closer, so the radius decreases. Atom--loses outer electrons-->Ion *Ion always smaller because it loses electrons**

What are Non-Metal Ions?

Atoms of non-metallic elements that tend to gain one or more electrons and form Anions (-). -One or more particle on the atom and electrons repel each other, so the radius increases. *Ion always larger because it has gained electrons**

What is Ionic Size?

Ionic Size is what tells us that: -CATIONS are always SMALLER than the atoms from which they form. -ANIONS are always LARGER than the atoms from which they form.

What is Ionization Energy?

The energy required to remove the most loosely bond, outermost electron from an element. -DECREASES from top to bottom within a group (LESS PULL/FARTHER) -INCREASES from left to right across a period (MORE PULL/CLOSER) *Opposite trend of Atomic Radius**

Down a Group:

As atomic size INCREASES, nuclear charge, ("power of the proton") has a smaller effect on the electrons in the highest occupied energy level. *Because of the increase in shielding effect** -The less energy is required to remove an electron, the lower the ionization energy. *More energy levels means less attraction between protons and electrons, so it would require less energy to remove an electron**

In a Period:

Ionization energy trends to increase from Left-->Right. *Nuclear charge, ("power of the proton") increases, but the shielding effect stays constant** -More energy is required to remove an electron as you go across. Ex.) It would require MORE energy to remove an electron from N than Li because there are more protons in N which means a stronger attraction between protons and electrons.

What is Electronegativity (EN)?

The ability of an element to attract electrons when the atom is in a compound.

What are some Trends in Electronegativity?

-Electronegativity values DECREASE down a group. -Electronegativity values tend to INCREASE across a period. -Increases from Fr/Cs in bottom left (lowest EN) to F in top right, (Highest EN) - 4.0. *The closer the element is to the Noble Gasses, the HIGHER the electronegativity**

What information can you find that would be helpful to this unit on Reference Table S?

Properties of Selected Elements [Ionization Energy, Electronegativity (EN), and Atomic Radius/Atomic Size]

RC.) Where are Electrons located?

Electrons are located on the orbitals or energy levels.

RC.) Which Electrons are involved in Chemical Reactions, and why?

The valence electrons are the only electrons involved in chemical reactions because the valence electrons are on the outermost orbitals and are readily available to be transferred or shared with other atoms.

RC.) What happens when an atom gains or loses electrons?

A neutral atom becomes an ion if it gains or loses electrons.

RC.) What is the maximum amount of valence electrons, and why?

The maximum amount of valence electrons is 8 because the OCTET RULE states that atoms tend to gain, lose, or share electrons in order to have a full set of 8 valence electrons.