Chemistry 1: Exam 3

Front 1

Two scientists that came to the same conclusion about how elements should be grouped.

Back 1

Dimitri Mendeleev and Lothar Meyer

Front 2

Three Periodic trends.

Back 2

Sizes of atoms and ions, ionization energy, and electron affinity

Front 3

Electron is both ______ to the nucleus, and _______ by other electrons.

Back 3

Attracted; repelled

Front 4

Define: Effective nuclear charge

Back 4

The net positive charge experienced by an electron in a many electron atom.

Front 5

Effective nuclear charge Zeff is found by: __________ (equation)

Back 5

Zeff= Z-s
(Z= atomic #, s= screening constant...close to the # of inner electrons)

Front 6

Bonding atomic radius is defined as...

Back 6

1/2 of the distance between covalently bonded nuclei

Front 7

Bonding atomic radius tends to ______ from left to right across a row due to ______ ______. And ________ from top to bottom of a column due to _______ ________ _______ ________.

Back 7

Decrease; increasing Zeff; increase; increasing value of n.

Front 8

Ionic size depends on what three things?

Back 8

Nuclear charge, # of electrons, orbitals in which electrons reside.

Front 9

________ are smaller than their parent atoms.

Back 9

Cations

Front 10

The outermost electron is ______ and _______ are _______.

Back 10

Removed; repulsions; reduced.

Front 11

______ are larger than parent atoms.

Back 11

Anions

Front 12

______ are added and _______ are _______.

Back 12

Electrons; repulsions; increased.

Front 13

______ increase in size as you go down a _______ due to _____ _____ _____ _____.

Back 13

Ions; column; increasing value of n.

Front 14

Define: Isoelectric series

Back 14

Ions have the same # of electrons.

Front 15

Ionic size ______ with an _____ _____ _____.

Back 15

Decreases; increasing nuclear charge.

Front 16

Define: Ionization energy

Back 16

Amount of energy required to remove an electron from the ground state of a gaseous atom or ion.

Front 17

What is the first ionization energy (I sub 1) define as?

Back 17

Energy needed to remove the first electron from a neutral atom.

Front 18

What is the second ionization energy (I sub 2) define as?

Back 18

Energy needed to remove the second electron.

Front 19

As one goes down a column ______ ______ is required to ______ the first electron.

Back 19

Less energy; remove.

Front 20

Atoms in the same group --->
______ is essentially the same, but ______ ______ are farther from the nucleus.

Back 20

Zeff; valence electrons

Front 21

Define: Electron Affinity

Back 21

Energy change accompanying addition of electron to gaseous atom.

Front 22

Trend in Electron Affinity -->
Electron Affinity becomes more ______ as you go from ______ to ______ across a row.

Back 22

Exothermic; left to right

Front 23

Metallic character increases from _____ to _____.

Back 23

Right to left

Front 24

What are the properties of metals?

Back 24

-Shiny 'metallic' appearance
-Solids at room temperature (except mercury)
-High melting points
-High densities
-Malleability is the ability of a metal to be hammered into shapes
-Ductility is the ability of a metal to be drawn into wire. -Because the valence electrons can move freely, metals are good heat conductors and electrical conductors.
-Tend to form cations in aq. solutions
-Most metal oxides are ionic solids that are basic.

Front 25

What are the properties of non-metals?

Back 25

-High ionization energies
-High electronegativities
-Poor thermal conductors
-Poor electrical conductors
-Brittle solids
-Little or no metallic luster
-Gain electrons easily

Front 26

Background of the Alkali Metals

Back 26

-Soft, metallic solids
-Arabic names
-Found only as compounds in nature
-Low melting points
-Low densities
-Low ionization energy
-Exothermic reactions
-All EXCEPT Li react with O2 to form peroxide

Front 27

Background of the Alkaline Earth Metals

Back 27

-Higher densities and melting points
-Low ionization but not as low as Alkali Metals
-Do not react with water.

Front 28

Background of Group 6A

Back 28

nonmetals= oxygen, sulfur, selenium
metalloid= tellurium
metal= polonium

Front 29

What are the oxygen allotropes?

Back 29

O2 and O3

Front 30

What are the three oxygen anions?

Back 30

O (above little 2-)= oxide
O2 (above little 2-)= peroxide
O2 (above little 1-)= superoxide

Front 31

What is Sulfur's most stable allotrope?

Back 31

S (sub 8)

Front 32

Describe group VIIA- Halogens

Back 32

-"salt formers"
-Large, negative electron affinities (oxidize easily)
-react directly with metals to form metal halides.

Front 33

Describe group VIIIA- Noble Gases

Back 33

-Astronomical ionization energies
-positive electron affinities
-monoatomic gases.

Front 34

Xe forms what 3 compounds?

Back 34

-XeF (sub 2)
-XeF (sub 4)
-XeF (sub 6)