WorksheetsUnit 2 Chem Test
Total questions: 66
Worksheet time: 54mins
Waves are defined by their _____ and ______.
(a)
As ______ increases, _____ decreases
(a)
_____ _____ recognized that electrons exist in definite energy states - called quantum states
(a)
_______ __ _____ theorized that since energy was proportional frequency (Planck’s Law) AND also proportional mass (Einstein’s E=mc2), frequency must also be proportional to mass.
(a)
_______ ______ recognizes that if you know the motion (momentum) of an object, it is impossible to know its position and vice versa
-If something is moving its position is changing and if you freeze an object, you change its motion
(a)
_____ ________ developed a probability equation to describe the position of an electron by treating it like a wave
(a)
The Wave Equation also predicts energy state – called “ (a) ” where electrons can be located
-No two electrons in the same atom can have the same set of four quantum numbers.
-Therefore, no two electrons in the same atom can have the exact same energy.
(a)
Waves are defined by their _____ and ______.
(a)
The orbitals are usually referred to by the letters s, p, d, f
s orbitals are ______ in shape and grow larger with increasing energy level
-Can “hold” two electrons
-s orbitals correspond to columns 1 & 2 on the periodic table
spherical
cubical
teardrop shaped
flat
p orbitals are shaped like _______ and fall along the x, y, or z axis
-There are 3 p orbitals in each energy level of 2 or higher
Can hold 6 total electrons
-p orbitals correspond to columns 13 through 18 on the periodic table
mirror tear drops
cubical
spheres
flat
There are five d orbitals
The d orbital can hold a total of _____ electrons
Corresponds to columns 3 – 12 on the periodic table
10
2
6
14
-There are 7 f orbitals of complex shapes that correspond to the lanthanide and actinide series
-Can hold __ electrons
10
2
6
14
The way electrons are distributed in an atom is called its ______ ________
(a)
The most stable organization is the lowest possible energy, called the _____ _____
(a)
The s and p blocks are called the _____ _____ ______
(a)
how many does s hold?
(a)
how many does p hold?
(a)
how many does d hold?
(a)
how many does f hold?
(a)
Before the developement of the periodic table, the known elements were grouped into random _____
lists
families
periods
charts
The first attempts at organizing the elements was made by ______ who noticed that he could make "triads" of three similar elements (like Li, Na, and K)
JW Dobereiner
John Newlands
Dmitri Mendeleev
Luthar Meyer
JW Dobreiner added that the average of masses of the lightest and heaviest was equal to the middle element.
What is this law known as?
Law of Triads
Hunds Rule
Law of Octaves
______ made similar groupings, but of eight elements with increasing masses
John Newlands
JW Dobreiner
Dmitri Mendeleev
Jacob Riis
_____ and ______ independently came to the same conclusion about how elements should be grouped
Dmitri Mendeleev
Lothar Meyer
JW Dobreiner
Jonathan Newland
Chemists mostly credit ____ because he also used chemical properties to organize the table and predicted some missing elements and their expected properties, including germanium
Mendeleev
Meyer
Dobreiner
Einstein
Mendeleev's table was based on _____ ____. It was the most fundamental property of elements known at the time.
Atomic Masses
Atomic Number
Atomic Radius
Ionic Measure
About 35 years later, the nuclear atom was discovered by ____ _____
Ernest Rutherford
Henry Moseley
JW Dobreiner
Eric Rutherford
_____ _____ developed the concept of atomic number experimentally. The number of protons was considered the basis for the periodic property of elements.
Henry Moseley
Ernest Rutherford
Henry Moose
Jonathan Newland
_____ is the repititve pattern of a property for elements based on atomic number.
Periodicity
Electron Affinity
Periodic Organization
Ionic Category
Many properties depend on attractions between ____ _____ and the _____
(a)
______ are both attracted to the nucleus and repelled by other electrons
The forces an electron experiences depend on both factors.
electrons
protons
neutrons
ions
The bonding atomic radius tends to
______ from left to right across a period
______ increase from top to bottom of a group
(a)
Sizes of ions are determined by _______ ______ in ionic compounds
interatomic distances
atomic distances
electronic distances
intergrating distances
Ionic size depends on
the nuclear charge
the number of electrons
the orbitals in which electrons reside
the number of protons
_____ are smaller than their parent atoms:
- The outermost electron is removed and repulsions between electrons are reduced
Cations
Anions
_____ are larger than their parent atoms
- Electrons are added and repulsions between electrons are increased
Cations
Anions
The ______ _____ is the minimum energy required to remove an electron from the ground sate of a gaseous atom or ion
ionization energy
electron affinity
electronegativity
atomic radius
The _____ ______ _____ is the energy required to remove the first electron
first ionization energy
ionization energy
second ionization energy
The _____ ______ _____ is the energy required to remove the second electron
first ionization energy
ionization energy
second ionization energy
The higher the ionization energy, the more (a) it is to remove an electron.
It requires ____ more energy to remove each successive electron
more
less
When all ______ have been removed, it takes a great deal more energy to remove the next electron (a core electron)
electrons
valence electrons
protons
neutrons
First Ionization Energy (I1)
I1 generally _____ across a period
I1 generally _____ down a group
(a)
_____ _____ is the energy change accompanying the addition of an electron to a gaseous atom
(a)
Electron affinity is typically _____, so, for most elements, it is negative!
exothermic
thermic
positive
negative
Group 2A
s sublevel is full
p sublevel is half-full
p sublevel is full
Group 5A
s sublevel is full
p sublevel is half-full
p sublevel is full
Group 8A
s sublevel is full
p sublevel is half-full
p sublevel is full
(a) is the ability of an atom in a molecule to attract electrons to itself.
On the periodic table, electronegativity generally (a) as you go:
-from left to right across a period
-from the bottom to the top of a group
Use final __ and __ to find valence electrons in an element
(a)
Alkali Family
1A
2A
6A
7A
8A
Alkaline earth Family
1A
2A
6A
7A
8A
Oxygen Family
1A
2A
6A
7A
8A
Halogens Family
1A
2A
6A
7A
8A
Noble gases
1A
2A
6A
7A
8A
The atomic radius decreases as we move across a period because
atomic mass increases
atomic number increases
effective nuclear charge increases
more electrons are added
The atomic radius increases as we move down the group because
atomic mass decreases
atomic number decreases
atomic number increases
number of shells increases
On moving across a period from left to right the ionisation energy increases because:
value of principal quantum number increases
effective nuclear charge increases
atomic size increases
nuclear charge increases
Why does nitrogen have higher ionisation energy than oxygen?
N: 1s2, 2s2, 2p3
O: 1s2, 2s2, 2p4
As we can see that Nitrogen has half filled p orbitals which is relatively stable configuration as compared to 2p4 configuration of Oxygen atom so it is difficult to remove one electron from this stable configuration. Further, removal of one electron from Oxygen atom is relatively easy because it results in half filled stable p orbital configuration. That's why ionisation energy of Nitrogen is more than Oxygen.
Why does beryllium have higher ionisation energy than boron?
As we move left to right in a period, ionization energy increases.
This is due to the addition of electrons in outermost shell and increasing stability to get noble gas configuration.
Berrylium has a stable configuration so it has higher ionization energy due to filled orbital.
Properties of metals include
*write down
form cations
lose e-
low in ie
solid at room temp
and
conduct electricity
ductile and malleable
Properties of nonmetals include
*write down
form anions
(-ions)
gain e-
HIGH in ie
gases or liquids or some solids
density varies
Properties of metalloids include
*write down
solids
metallic lustre
brittle and easily broken
ability to conduct electricity but not as well
make sure to copy down chart with families
