Unit 5 Chem Test
Explain why the elements in the "dip" (Group 3-12) only have 2 valence electrons
The elements in the dip only have 2 valence electrons because transitional metals may have subshells that aren't all the way filled. An atom could accept or lose electrons from an incomplete subshell if that makes a full subshell and then they behave like valence electrons.
Describe the properties of noble gases (make sure to explain how helium is different than the rest of its family.)
They are all odorless, colorless gases with a low chemical reactivity. They have a complete octet because they have all 8 possible electrons. Helium is different than the rest of the noble gases because it only have 2 valence electrons while the rest have 8. *inert- non-reactive - gases are only element with 3 stages.
member of the transition metal family
Zn
what classifies a "block" on the periodic table?
a block on the periodic table is a group of elements that have the same number of orbitals
atomic radius
a measure of the size of its atoms or the normal distance from the nucleus to the surrounding shell of the atom; estimated size of atom - going left to right the atomic size decreases -going from top to bottom the atomic size increases
anion
a negatively charged ion ( more electrons than protons) (gains electrons so is larger than parent atom)
cation
a positively charged ion (more protons than electrons) (loses electrons so is smaller than parent atom)
Identify the name given to the first group on the periodic table (group 1)
alkali metals
describe how elements in the same row are similar
all the elements in the same row are similar because they have the same number of electron shells. As you move to the right of the row, each element has one more proton and is less metallic than the previous one
identify the liquids on the periodic table
bromine, mercury, caesium, gallium, rubidium, francium
oxidation numbers
charge that the atom will have when it forms an ion
He was able to use his periodic table to predict ____________________ of the missing elements
chemical properties
Mendeleev was able to use his periodic table to predict___________ of the missing elements.
chemical properties
describe the trend for electron affinity as you go across the periodic table and as you go down the periodic table
electron affinity increases across the periodic table and can decrease when you go down the periodic table - pattern goes left to right except noble gases
the attraction an atom has for electrons is called
electronegativity
elements in the same row on the periodic table have the same number of
energy levels
a column on the periodic table is called a
family
Columns are called ___________ or ________________.
family or groups
elements in the Noble Gas family are considered stable because they have _________ valence levels
full (filled)
octet rule
goal of atoms to have 8 valence e- (except tiny atoms only need 2 e-) *makes them stable
identify all the gases on the periodic table
helium, argon, krypton, neon, kenon, radon, hydrogen, oxygen, nitrogen, florine, and chlorine
the second row of the f-block are known as the
inner transition metals
the amount of energy required to remove an electron from a neutral atom is called ___________
ionization energy
describe the trend for ionization energy as you go across the periodic table and as you go down the period table
ionization energy increases from left to right and decreases as you go down the periodic table
the first row of the f-block are known as the
lanthanides and actinides
A negative ion is (larger/smaller) than its parent atom
larger
Where are the most active metals located?
lower left
describe the trend for metallic character as you go from left to right across the periodic table and as you go down a group (from top to bottom)
metallic character decreases as you go from left to right across the periodic table and increase as you move down element groups in the periodic table
elements that have characteristics of both metals and nonmetals are called
metalloids
is a negative ion larger or smaller than their neutral atom
much larger than their neutral atom
Identify the name given to group 18 on the periodic table
noble gases
where are all of the metals on the periodic table located?
on bottom left
identify where each of the following blocks are on the periodic table
s-block-> the 1st columns on the left (group 1 and 2) p-block-> the right side of the table (groups 13 to 18) d-block-> the middle of the table (group 3 to 12) f-block-> at the bottom 2 rows of the periodic table
A positive ion is (larger/smaller) than its parent atom
smaller
is a positive ion larger or smaller than their neutral atom
smaller than their neutral atom
all of the rest of the elements on the periodic table are
solids
describe the properties of alkali metals
the alkali metals are shiny, soft, really reactive metals at standard temperature. They often lose their outermost electron and form catons.
How is this table arranged (current periodic table)?
the current table is arranged by increasing atomic numbers.
Describe how elements in the same column are similar
the elements in each group have the same number of electrons in the outer orbital. the electrons in each column all have the same number.
electron affinity
the energy change that occurs when an atom or ion gains an electron
ionization energy
the minimum amount of energy required to remove the most loosely bound electron of the neutral gas atom - going left to right the ionization energy increases - going top to bottom ionization energy decreases
ionic radius
the radius of a monatomic ion in an ionic crystal structure. It is the radius of an ion (anions or cation) estimated size of an ion
Groups 3-12 are called
transition metals
Where are the most active nonmetals located?
upper right
describe the properties of nonmetals
-dry brittle, poor conductors of heat/electricity -not magnetic -makes dull sound when they are hit -not very strong and has low density
forms 3+ ions when bonding
Al
what elements are considered metalloids
Boron, Silicon, Antimony, Tellurium, Germanium, Polonium, Arsenic
gas at room temp
Cl
gas at room temperature
Cl
who created the first periodic table?
Dimitri Mendeleev
Identify the name given to Group 17 on the periodic table
Halogens
group 17 is called
Halogens (halides)
_____________ discovered that each element has a unique atomic number and arranged the elements in order or increasing atomic number
Henry Mosley
electron distribution ending in s1
K
metal
K
member of the alkali metal family
Li
highest ionization energy
N
8 valence electrons
Ne
smallest atomic radius
Te
How is the extended periodic table different from the one we are used to seeing? Why don't we usually draw it this way?
The extended periodic table has theories of chemical elements beyond what is on the normal periodic table. The extended periodic table is a lot larger and we don't draw it this way due to uncertain and variability of the properties of elements passed 120.
Periodic Law
The law says that the properties of the element are periodic functions of their atomic numbers. This means that the chemical and physical properties of elements are periodic when their atomic weights are in order.
electronegativity
a chemical property which declares the propensity on an atom to attract an electron. The strength of an atom to hold onto its electrons when the atom is interacting with other atoms.
first group on periodic table
alkali metals
second group on periodic table
alkaline earth metals
_______________ is defined as one half the distance between nuclei of two like atoms
atomic radius
As you go down a group, the first ionization energy generally ( decreases/increases)
decreases
As you go from left to right across a period, the atomic size (decrease / increase) Why
decreases nuclear charge
As you travel down a group, the atomic size (decrease/increase) why
increase energy
As you go from left to right across a period, the first ionization energy generally (decreases/increase) Why
increase positive charge
describe the trend for atomic radius as you go from left to right across the periodic table and as you go down a group (from top to bottom)
increases as the group and energy level increase but it decreases as you move across the periodic table
describe the properties of metalloids
look like metals but behave like non-metals. they are shiny and brittle with pretty good conductivity. properties of both - top and bottom
the s and p-blocks together are called the
main group elements
where are the nonmetals located on the periodic table?
on the upper right of the periodic table
The _______________________ states that properties of elements repeat when arranged by increasing atomic number
periodic law
rows are called ________
periods
the d-block is known as the
transition elements
describe some characteristics of the transition elements:
-good conductors of heat/electricity - (malleable) be bent into shape/hammered easily -high melting points -ductile (drawn to wires) -multi valent levels -produce color in (aq) solution
Identify the name given to the 2nd group on the periodic table (group 2)
Alkaline Earth Metals
Describe the properties of Alkaline Earth Metals
All of the alkaline earth metals are shiny, silvery/white, and can be reactive metals when it is standard temp and pressure.
Group 13 is called
Boron Family
4 valence electrons
C
group 14 is called
Carbon Family
largest atomic radius
Cc
compare hydrogen to the alkali metals (similarities and differences)
Differences: -hydrogen is a very reactive gas -alkali metals are even more reactive -hydrogen is a non metals and can form ionic cation compounds while Alkali only can form ionic compounds Similarities: - both 1 valence e- - both gases - both form a cation when they rise an electron.
_____________ arranged th periodic table in order of increasing atomic mass
Dimitri Mendeleev
higher electronegativity
F
highest ionization energy
F
Which element has the highest electronegativity?
Fluorine
Describe the properties of Halogens
Form stable compounds with both metals and nonmetals. they are the most reactive non-metal elements. This is because they have 7 valence electrons and only needed for a full octet.
member of the noble gas family
He
How did Mendeleev organize his periodic table?
He arranged the periodic table in order of increasing atomic mass.
Who rearranged the periodic table?
Henry Mosley
liquid at room temperature
Hg
member of the Halogen family
I
Group 15 is called
Nitrogen Family
group 18 is called
Nobel gases
forms 2- ions when bonding
O
group 16 is called
Oxygen Family (chalogen)
3 energy levels
S
metalloid
Sb
