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148 Cards in this Set

  • Front
  • Back
How are elements ordered in the modern periodic table?
According to increasing atomic number.
Mendeleev noticed that certain similarities in the chemical properties of elements appeared at regular intervals when the elements were arranged in order of increasing _________.
Atomic mass.
What does the modern periodic table state?
The physical and chemical properties of an element are functions of its atomic number.
What did the discovery of the noble gases do?
Changed Mendeleev's periodic table.
How did the discovery of the noble gases change Mendeleev's periodic table?
It added a new group.
What is the most distinctive property of the noble gases?
They're largely unreactive.
If an isotope of fluorine has a mass number of 19 and an atomic number of 9. How many protons and neutrons are in this atom?
9 Protons.
10 Neutrons.
An isotope contains 53 protons, 78 neutrons, and 54 electrons. What is the atomic number? Mass number?
The atomic number is 53, and the mass number is 131.
Is a period of the periodic table horizontally placed or vertically placed?
Horizontally.
Is a group/family of the periodic table horizontally placed or vertically placed?
Vertically.
What is atomic mass?
The mass of the atom.
What is atomic number?
The number of protons in the nucleus of an atom.
What did Mendeleev do that was so monumental?
He arranged elements in order of various properties and created the first periodic table, published in 1869.
Who created periodic law?
Mendeleev.
Who improved Mendeleev's law?
Mosley.
State the periodic law.
The chemical and physical properties of elements are periodic functions of their atomic number.
What happens when elements are arranged in order of increasing atomic number?
Elements with similar properties appear at regular intervals.
What is an arrangement of elements in order of atomic numbers so that elements with similar properties fall in the same column/group?
The periodic table.
Noble gases are ________. (Unreactive or Reactive.)
unreactive
Who discovered the noble gases?
John William Strutt & Sir William Ramsey the first.
What is periodicity?
Similar trends between elements.
Noble gases undergo few chemical reactions.

True or False?
True.
For each period, how many elements are in each?
2 in Period 1.
8 in Period 2.
8 in Period 3.
18 in Period 4.
18 in Period 5.
32 in Period 6.
32 in Period 7.
For each period, in what order do the sublevels fill?
1s in Period 1.
2s2p in Period 2.
3s3p in Period 3.
4s3d4p in Period 4.
5s4d5p in Period 5.
6s4f5d6p in Period 6.
7s5f6d7p in Period 7.
How do you find period from electron configuration?
Take the highest number. (NOT exponent.)
What determines which block an element is in?
The highest letter it contains. (s,p,d,f)
What are the two exceptions to "block theory"? Why?
He & H because of differing properties.
What are group one elements?
Alkali metals.
Alkali metals have a _______ appearance and are ______.
silvery, soft
Are s-block elements chemically reactive metals?
Yes.
Group two elements are ___________ metals.
alkaline-earth
Group two elements are ______, denser, & _________ than alkali metals.
harder, stronger
What do alkaline-earth metals contain?
A pair of electrons in their outermost sublevel.
What does each d sublevel consist of?
5 orbitals with a maximum of 2 electrons each.
Which block consists of transition metals?
The d-block.
Transition metals are metals with typical ______ properties, they are ____ conductors of electricity, and they have _____ luster.
metallic, good, high.
Transition metals are relatively _______. (Reactive/Unreactive.)
unreactive
The d-block contains groups _-__.
3, 12
The p-block contains groups __-__.
13, 18
The s-block contains groups _-_.
1, 2
p-block elements + s-block elements = _______ elements
main group
The total number of electrons in atoms of the p-block in the highest occupied level is equal to what?
The group number minus ten.
Elements in the p-block vary in ______.
properties
The right-hand end of the p-block contains all of the ______, except for H & He.
nonmetals
All six metalloids are in the _-block.
p
Which group are halogens a part of?
Group 17.
Halogens are the most reactive ________.
nonmetals
P-block elements are _______ than s-block elements, but _______ and _____ dense than d-block.
harder, softer, less
_______ is the exception to p-block rules, because it's reactive.
Bismuth
F-block elements are ________ and _______.
lanthanides, actinides
______ elements are wedged between groups 3 & 4 and periods 6 & 7 on the periodic table.
F-block
There are ___ f-block elements between La& Hf called _______.
14, lanthanides
Lanthanides are _______ and similar in _______ to alkaline earth metals.
shiny, reactivity
14 f-block elements between Ac & Rf called actinides, and they are _____.
radioactive
The first four actinides, Th-Np are _____ the rest are ________.
natural, created in laboratories
The size of an atom is defined by it's what?
Orbital's edge.
What is atomic radius?
Half the distance between the nuclei of identical atoms that are bonded together.
From left to right, atomic radii ______ on the periodic table
decreases
How is the trend of smaller atoms across a period caused?
By the increasing positive charge of the nucleus.
Name the noble gases in order.
He, Ne, Ar, Kr, Xe, and Rn.
As electrons add to s and p sublevels, they are gradually pulled closer to the higher charged nucleus, resulting in a _______ in atomic radii.
decrease
The atomic radii of main group elements normally ________ down a group.
increases
How can an electron be removed from an atom?
If enough energy is supplied.
A + energy ---> A+ + e-

Label this.
A = symbol of any element.
A+ = ion or A with a positive charge.
What is an ion?
An atom/group of bonded atoms that has a positive or negative charge.
What kind of ion does Sodium form?
Na+
What is ionization?
Any process that results in the formation of an ion.
What is ionization energy? (IE)
The energy required to remove one electron form a neutral atom of an element.
Why are measurements of ionization energies made on isolated atoms in the gas phase?
To avoid influences from nearby atoms.
What are ionization energies measured in?
kj/mole
Ionization energies ________ with groups like H-Cs.
decreases
Group one metals have the ________ first ionization energies in their respective periods.
lowest
The higher the reactivity of a metal, the _______ electron loss is.
easier
Ionization energies of main group elements ________ across each period.
increase
Ionization energies of main group elements _______ across each period.
increase
Why do ionization energies of main group elements increase across each period?
Because of the increasing nuclear charge.
A ______ charge attracts electrons in the same energy level. (Ionization energies.)
higher
What is responsible for both increasing ionization energies and decreasing atomic radii across periods?
Increasing nuclear charge.
Generally, nonmetals have higher ___________ than metals.
ionization energies
Group 1 has the ______ ionization energy and an element of Group 18 has the _______.
lowest, highest
Among main group elements, ionization energies generally ______ down the groups.
decrease
As atomic number increases going down a group, _______ lie between the nucleus and the electrons in the highest occupied energy levels.
electrons
How can electrons can be removed from positive ions as well as from neutral atoms?
Sufficient energy must be supplied.
The energies for the removal of additional electrons from an atom are referred to as the what?
Second ionization energy (IE2), third ionization energy (IE3), and so on. (*)
The second ionization energy is always ____ than the first, third is _____ than second, etc.
higher, higher
Why do fewer electrons remain within the atom to shield the attractive force of the nucleus? (Ionization energies.)
Because electrons are removed in successive ionizations.
Each successive electron removed from an ion feels an increasingly _______ effective nuclear charge. (The nuclear charge minus the electron.)
stronger
Removing a single electron from an atom in of a group 18 element is ______ than removing an electron form atoms of other elements in the same period. (Harder or easier?)
harder
Can neutral atoms acquire electrons?
Yes.
What is called the atoms electron affinity?
The energy change that occurs when an electron is acquired by a neutral atom.
What do most atoms do when they acquire an electron?
Release energy.
Some atoms must be "forced" to gain an electron by the _____ of energy.
addition
Elements are more likely to form what kind of ions with lower ionization energies?
Positive.
Ions are very ______ making their electron affinity is very hard to determine.
unstable
Electron affinity is measured in ______.
kJ/mole
______ gain electrons the most often.
Halogens
Generally, as electrons add to the same p sublevel of atoms with increasing nuclear charge electron affinities become more ______ across each period within the p- block. (Groups 14-15 are exceptions.)
negative
Outer level electrons are what kind of electrons?
Valence.
Lanthinides and Actinides are in group 3.

True or False?
False, they are groupless.
Ca+ _____ an electron.
removes
Ca- ______ an electron.
adds
O2- adds _____ electron(s).
2.
Electrons typically _______ down a group in electron affinities.
decrease
A slight increase in effective nuclear charges down a group ______ electron affinities.
increases
An _______ in atomic radius down a group decreases electron affinities.
increase
Exceptions to group trends in electron affinities are _______________, which tend to be the same size or even decreasing down a group.
heavy transition metals
Certain p-block nonmetals tend to form _____ ions.
negative
Group 16 elements are present in many compounds as __ ions, (O, which sometimes achieves the configuration of Ne.)
2-
What is a positive ion called?
A cation.
The formation of a cation by the loss of 1+ electron always leads to what? Why? What happens to the remaining electrons?
A decrease in atomic radius. Because of the removal of the highest energy level electrons results in a smaller electron cloud. They're drawn closer to the nucleus by its unbalanced negative charge.
What is a negative ion called?
An anion.
How are anions formed?
By the addition of one or more electrons.
What does the formation of anions lead to?
An increase in atomic radius.
Why does the formation of anions lead to an increase in atomic radius?
Because the total positive charge of the nucleus remains unchanged when an electron is added to the atom/ion therefore electrons are not drawn to the nucleus as strongly as they were before the addition of the extra electron.
Why does the electron cloud spread out when anions are formed?
Because of greater repulsion between the increasing number of electrons.
Metals at the left end of the table form ______.
cations
Nonmetals at upper right tend to form ________.
anions
Do cationic radii decrease or increase across a period? Why?
Decrease. Because the electron cloud shrinks due to increasing nuclear charge acting on the electrons in the same main energy level.
Starting in Group __, anions are more common than cations.
15.
Why does anionic radii decrease across each period for the elements in Group 15-18?
The same reason why carionic radii decrease from left-right across a period.
Outer electrons in cations and anions are in ______ energy levels as one reads down a group.
higher
There is a gradual _______ of atomic radii down a group, there's also a gradual ______ of ionic radii.
increase, increase
Why do chemical compounds form?
Because electrons are lost, gained, or shared between atoms.
What are electrons that are available to be lost, gained, or shared in the formation of chemical compounds?
Valence electrons.
Where are valence electrons often located?
In incompletely filled main energy levels.
The electron lost between Na & Na+ is what kind?
A valence electron!
Main group elements' valence electrons are in the ________ s & p sublevels.
outermost
Respectively, Group 1 & 2 elements have ____ or ____ valence electrons.
one, two
Elements of Groups 13-18 have a number of valence electrons equal to what?
The group number minus 10.
Sometimes both s & p sublevel valence electrons of the p-block are involved in compound form.

True or False?
True.
Valence electrons hold atoms together in what?
Chemical compounds.
Who devised a scale of numerical values reflecting the tendency of an atom to attract electrons?
Linus Pauling.
What is electronegativity?
A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.
What is the most electronegative element? (4)
Fluorine.
Electronegatives tend to _______ across each period.
increase
Aklaki and alkaline-earth metals are the ______ electronegative elements.
least
Electronegatives tend to _______ down a group or remain about the same.
decrease
Why are the noble gases not assigned electronegativity?
Because they do not form compounds.
When a noble gas does form a compound, its electronegativity is extremely ____, similar to halogens.
high
Where are the elements with the highest electronegativity located on the periodic table?
The upper-right.
Where are elements with the lowest electronegativity located on the periodic table?
The lower-left.
D-block elements are all ______.
metals.
Ionization energies of the f-block and d-block elements generally _______ across the periods.
increase
The first ionization energies of the d-block elements generally ______ down each group.
increase
Why do the first ionization energies of the d-block elements generally increase down each group?
Because the electrons available for ionization in the outer s sublevels are less shielded from the increasing nuclear charge by electrons in the incomplete (n-1)d sublevels.
Among all the atoms of the d-block and f-block elements, electrons in the highest occupied sublevel are always removed ______.
first
Most d-block elements commonly form ____ ions in compounds
2+
Only the active metals of Groups __-__ have low electronegatives.
1, 2