Chemistry Ch. 5
by increasing atomic numbers
After many years of study and revisions, how is the periodic table arranged today?
Cations (less electrons) tend to be smaller than anions (more electrons) tend to be larger
Are cations or anions smaller than neutral atoms?
Ne
Neon
1. metallic luster 2. crumbly, brittle solids 3. conduct electricity better than nonmetals but not as well as metals
What are some characteristics of metalloids?
1.generally gases or soft, crumbly solids 2. Bromine is a liquid 3. Diamond is the hardest known natural substance 4. generally poor conductors of thermal energy and electrical current
What are some characteristics of nonmetals?
Group 7A, because it will add one electron instead of loosing 7 electrons
Which group 1A or 7A has a higher electron affinity?
Group 7A
Which group 1A or 7A has a higher ionization energy?
because the strength with which protons in the nucleus attract the outer-shell electrons increases
Why does the ionization energies generally increase from left to right across a period?
Antoine Lavoisier
a French chemist that used the word "element"
Dmitri Mendeleev
a Russian chemist who established the structure of the modern periodic table, but arranged the elements by their atomic mass and left blanks for elements he believed were not yet discovered; he also included transition elements
International Union of Pure and Applied Chemistry (IUPAC)
a convention of numbering the columns from 1 through 18; each family is uniquely identified
periodic table
a description of how elements differ from one another
paramagnetic
a property of materials that are weakly attracted by a magnetic field because of unpaired electrons
Al
aluminum
Henry Moseley
an English physicist who found the elements are related to the number of protons in the nucleus (atomic number)
B
boron
F
fluorine
Hg
mercury
Mo
molybdenum
Ni
nickel
N
nitrogen
atomic number
the number of protons
it decreases
Does the atomic radius increase or decrease as you move across the periodic table from left to right?
it increases, because another principal energy level is added
Does the atomic radius increase or decrease as you move down a column in the periodic table?
left to right
Does the electronegativity of the elements increase as you move from left to right on the periodic table or right to left?
1. element's atomic number 2. element's name 3. element's symbol 4. element's atomic mass 5. element's electron configuration 6. element's physical properties
On the periodic table, for each element, what information is given?
1. has one electron 2. reacts like other Group IA elements 3. also similar to Group 7A elements because it only needs one more electron to fill its outer shell 4. combines with many elements to form compounds 5. forms, with carbon, hydrocarbons
What are some chemical properties of Hydrogen?
1. colorless, odorless, tasteless 2. diatomic molecule
What are some physical properties of Hydrogen?
1. very reactive 2. typically form cations (+1) 3. conduct heat and electricity well 4. metallic luster 5. low densities and soft 6. must be stored in oil
What are some properties of alkali metals?
1. metallic luster 2. crystalline and brittle 3. lower ductility and malleability than metals 4. semiconductors
What are some properties of metalloids?
1. solid at room temperature 2. denser, harder, and have higher melting points than the alkali metals 3. form cations (+2) 4. malleable 5. typically donate their 2 valence electrons
What are some properties of the alkaline-earth metals?
1. paramagnetic 2. when cut, bright and silvery 3. usually give up their 2 valence electrons 4. actinide series are radioactive and used in nuclear power plants
What are some properties of the inner transition metals?
1. high densities 2. hard, tough, and strong 3. shiny luster 4. conduct heat and electricity well 5. ductile and malleable 6. 2/3 are native minerals
What are some properties of the transition metals?
1. used to manufacture ammonia used in crop fertilizers 2. the space program for rocket fuel 3. hydrogenation (forms semi solid fats) 4. in the future, fuel cell technology
What are some uses of hydrogen?
1. solid 2. lustrous (shiny) 3. malleable (shapeable) 4. ductile 5. good conductors of heat and electricity (some exceptions: mercury is a liquid and manganese is a brittle solid)
What are the characteristics of most metals?
post-transition metals
What are the metals in Groups 13-16?
transition metals
What are the metals in groups 3-12?
oxygen
What element is a member of both Period 2 and Group 16 (6A)?
calcium
What element is a member of both Period 4 and Group 2 (2A)?
indium
What element is a member of both Period 5 and Group 13 (3A)? use pgs. 108-109
The Boron Family (3 valence electrons)
What is the name of Group 13 (3A)?
The Carbon Family (4 valence electrons)
What is the name of Group 14 (4A)?
The Nitrogen Family (5 valence electrons)
What is the name of Group 15 (5A)?
The Oxygen Family (6 valence electrons)
What is the name of Group 16 (6A)?
The Halogen Family (7 valence electrons)
What is the name of Group 17 (7A)?
The Noble Gas Family (8 valence electrons)
What is the name of Group 18 (8A)?
alkali metals
What is the name of Group 1A?
alkaline-earth metals
What is the name of Group 2A?
Period 4 and Group 1 (1A)
What period and family is the element potassium found in?
Period 3 and Group 16 (6A)
What period and family is the element with the atomic mass of 32.07u found in?
Period 3 and Group 17 (7A)
What period and family is the element with the atomic number 17 in?
They do not except unless under unusual conditions of pressure and temperature.
When do noble gases react with other elements?
1. small amounts in the earth's atmosphere 2. large quantities are contained in gaseous byproducts of fuel and other refining processes, separated by electrolysis 3. from heated coke (impure carbon obtained from coal)
Where is hydrogen found?
group or family
a vertical column of elements on the periodic table; have similar physical and chemical properties due to their electron configuration
Ar
argon
metalloids
around the stair-step line between the cells in Groups 13-17
As
arsenic
Ba
barium
Be
beryllium
Br
bromine
Ca
calcium
C
carbon
Cs
cesium
Cl
chlorine
Cr
chromium
Co
cobalt
physical properties
colors and icons give information about the physical properties of he element, such as whether it is a metal or nonmetal and whether it is radioactive
hydrocarbons
compounds formed when hydrogen atoms and carbon atoms form compounds
Cu
copper
John Dalton
documented a list of sixty elements
representative groups
elements in the s and p blocks of the periodic table; designated with A suffixes in the North American Convention Periodic Table
native minerals
elements that are found as pure solids in nature
transition elements
elements that do not fit into the major families, but they all have similar chemical and physical characteristics
transuranium elements
elements with atomic numbers greater than 92 (Uranium's atomic number); except for neptunium and plutonium, all are products of artificial processes in nuclear reactors or bomb explosions
actinide series
fits into the table after actinium; placed at the bottom of the table; their interior f sublevel electrons are added with increasing atomic number
Ga
gallium
Ge
germanium
Au
gold
North American Convention Periodic Table
has a combination of Arabic numerals and letters that are placed above each column to indicate the valence electron structure of the elements in each column
symbol
has one, two, or three letters; most prominent item in the cell
He
helium
periods or series
horizontal rows of elements; indicates the highest principal energy level that electrons occupy in ground-state atoms
H
hydrogen
lanthanide and actinide series
inner transition metals
I
iodine
Fe
iron
Kr
krypton
Pb
lead
Li
lithium
Mg
magnesium
Mn
manganese
metals
on the left side and the middle of the periodic table
nonmetals
on the right side of the periodic table; separated from the metals by a stair-step line
John Newlands
organized elements by their atomic mass; used octaves, which was not well received
O
oxygen
P
phosphorous
lanthanide series
placed at the bottom of the table; their interior f sublevel electrons are added with increasing atomic number; fits in the table immediately after the element lanthanum
Pt
platinum
Pu
plutonium
K
potassium
Ra
radium
Rn
radon
Rb
rubidium
Se
selenium
Si
silicon
Ag
silver
Na
sodium
periodic law
states that the properties of elements vary with their atomic numbers in a periodic way; formulated by Mendeleev and later revised by Moseley
Sr
strontium
S
sulfur
electron affinity
the amount of energy required to "add" an electron to a neutral atom to form a negative ion, or anion; opposite of ionization energy; depends on the size of the atom and the fullness of the highest energy sublevels; the energies becomes larger from left to right along a period
atomic radius
the distance from the center of an atom's nucleus to its outermost electron; determined by the electron cloud that surrounds the atom; the measure of an atom's size
metalloids
the elements immediately adjacent to the stair-step line; share properties of metals and nonmetals
hydrogen
the lightest element and the most abundant in the entire universe; often considered a family by itself
electronegativity
the measure of the attraction between the nucleus and valence electrons; the atom's ability to attract and hold electrons in a "molecule"; plays a central role in predicting how atoms chemically combine with each other
first ionization energy
the minimum energy required to remove the first electron from its outermost shell to make a cation; how easily electrons are "taken away" from atoms to form cations; generally increases from left to right within a period and decreases from top to bottom within a group
electron configuration
the number and location of electrons in each occupied energy level in the neutral atom; listed below the atomic mass
descriptive chemistry
the study of elements and the compounds they form
atomic mass
the weighted average located under the symbol
Sn
tin
Ti
titanium
U
uranium
Johann Dobereiner
used triads (groups of three elements with similar properties); his method was a step that lead to periodicity
sulfides
when certain metals combine with sulfur to form compounds
oxides
when oxygen combines with other elements to form a compound
periodicity
when some measurable property repeats on a regular basis in a sequential list or time sequence
Xe
xenon
Zn
zinc