Chemistry - Periodic Trends - Chapter Review
Everyone wants that full complement of eight outer electrons, what is this called.
Rule of Eight or Electron Octet
s orbitals have a spherical shape and can hold how many electrons each?
S orbitals have a spherical shape and can hold 2 electrons each.
S sublevels can hold how many electrons each?
S sublevels can hold 2 electrons each
Alkali Metals and Alkaline Earth Metals are part of what Block Elements
S-Block Elements
A combination of a metal and a halogen
Salt
How many electrons will be gained or lost by Selenium when forming an ion?
Selenium (Se) gains two electrons to form the selenide anion Se2- (2 is superscript)
Which of the following elements is (are) classified as metalloid: Silicon (Si), Phosphorus (P), and Sulfur (S)
Silicon (Si)
Which has a stronger electron affinity, Silicon or Barium?
Silicon has a stronger electron affinity Electron affinity tends to increase from left to right; Silicon is to the right of Barium on the periodic table.
Electronic configuration of Silicon
Silicon, Si Ne3s²3p² After 2p fills up, the lowest-energy orbital is 3s, in the third shell, followed by 3p
Neon has ten electrons. The order of filling its subshells is first 1s, then 2s, and finally 2p. What is the order of filling the subshells in an atom of magnesium (Mg)? (Use the periodic table to determine the number of electrons in an atom of magnesium)
Since there are 12 electrons in an atom of Magnesium, the order of filling of the subshells is 1s2s2p3s
Electronic configuration for Sodium
Sodium, Na Ne3s¹ Sodium, Ne we can write this as Ne3s¹, indicating one s electron orbiting outside a group of electrons just like Neon's. After 2p fills up, the lowest-energy orbital is 3s, in the third shell, followed by 3p
What are the properties of Alkali Metals
Soft enough to cut with knife; contain 1 valence electron
Sometimes atoms share electrons, and these shared electrons are attracted to both what?
Sometimes atoms "share" electrons, and these shared electrons are attracted to both nuclei. This attraction acts like glue to hold the atoms together to form molecules.
Alklai metals are located where on the period table
Starting on the far left of the periodic table
We can also identify an atom if we are given its electron configuration. For example, this configuration 1s²2s²2p⁶3s²3p¹ has 13 electrons. Only the aluminum atom has 13 electrons; therefore, the configuration above must be that of an aluminum atom. What atom has this electron configuration? 1s²2s²2p⁶3s²3p⁴
Sulfur (S (2+s+6+2+4=16)
Electronic configuration of Sulfur
Sulfur, S Ne3s²3p⁴ After 2p fills up, the lowest-energy orbital is 3s, in the third shell, followed by 3p
What is a great example of a Alkali-Halogen Compound?
Table Salt NaCl
Elements within a group tend to have the same number of valence electrons and for that reason what?
Tend to have similar chemical properties
For Transition Metals, what happens to electrons in bonding?
Tend to lose electrons to become positively charged ions
The Superscripted numbers and signs in the atoms' symbols indicate the ion's overall what?
The Superscripted numbers and signs in the atoms' symbols indicate the ion's overall charge
What is one of the most important concepts in this chapter according to the PowerPoint?
The Trends
Electronegativity
The ability of an atom in a compound to attract electrons from another atom in the compound.
Electronegativity What is it according to the PowerPoint?
The ability of an atom in a compound to attract electrons from another atom in the compound.
The d orbitals have a cloverleaf shape and there are how many on each d sublevel?
The d orbitals have a cloverleaf shape and there are 5 on each d sublevel.
Electron Affinity
The difference in energy when an electron is added to a neutral atom.
Electron Affinity What is it according to the PowerPoint?
The difference in energy when an electron is added to a neutral atom.
Orbitals
The electron configurations within each energy level Note: named no doubt by nostalgic physicists dreaming of planets
The elements within a group tend to have the same number of what?
The elements within a group tend to have the same number of valence electrons and for that reason tend to have similar chemical properties.
Ionization Energy
The energy needed to remove an outer electron - depends on atom's size
Ionization Energy What is it according to the PowerPoint?
The energy required to remove one electron from the outer shell of an atom (Ion - an atom or group of elements that bears a positive or negative charge)
Ionization Energy
The energy required to remove one electron from the outer shell of an atom.
The f orbitals have a double cloverleaf shape and there are how many on each f sublevel?
The f orbitals have a double cloverleaf shape and there are 7 on each f sublevel.
Atomic Radius
The geometric size (not the mass) of the atoms
The last column on the periodic table is uniquely strange. How does that relate to their ionization energies.
The last column of the periodic table is uniquely strange, because they live far to the right and have high ionization energies, so they don't easily make cations.
The last column on the periodic table is uniquely strange. How does that relate to their electron affinity.
The last column of the periodic table is uniquely strange, because they live far to the right....They also have low electron affinity because their outer orbital shells are full so they don't make anions either.
The most complicated orbitals are what?
The most complicated orbitals we will consider are called d orbitals
The names of d orbitals come from the details of what?
The names of the d orbitals come from the details of quantum mechanics
The next simplest orbitals are called what?
The next simplest orbitals are called p orbitals.
Why are the noble gases referred to as "noble"?
The noble gases are described as "noble" because they seem to consider it beneath themselves to react with other elements. Because these elements have completely filled valence shells, they have no energetic reason to react. They're already stable as they can be.
P orbitals have a dumbbell shape and there are how orbitals on each p sublevel?
The p orbitals have a dumbbell shape and there are 3 orbitals on each p sublevel.
The periodic table is broadly divided along a stairstep border into what?
The periodic table is broadly divided along a stairstep border into metals and nonmetals, with a few confused "metalloids" straddling the fence
Certain properties are characteristic of metals. Metals are usually malleable (can be beaten into fine sheets) and ductile (can be drawn into wires). Gold leaf is a very thin sheet of gold. In making gold leaf, we are using what common property of metals?
The property of malleability
Ionic Radii
The radii of the most common ions of the elements
Ionic Radii What is it according to the PowerPoint?
The radii of the most common ions of the elements. -Positive ions - cations -Negative ions - anions
Can a lower shell have higher energy than a higher number shell?
The shells have overlapping energies: e.g. some orbitals is shell4 (rd adn 4f) have higher energy than some orbitals in shell 5 (5s), even though 4 is "lower" than 5
What is the shape of a s orbital?
The simplest kind of orbital is called an s orbital and is shaped like a sphere.
What is the simplest kind of orbital?
The simplest kind of orbital is called an s orbital and is shaped like a sphere.
There are three different kinds of p orbitals. What are they.
There are three different kinds of p orbitals. Each kind points in a different direction, and each one is perpendicular to the others Examples -2px (x is subscript) (oriented along the x axis) -2py (y is subscript) (oriented along the y axis) -2pz (z is subscript) (oriented along the z axis)
Generally describe the Alkali Metals
These most metallic of the elements are very reactive, meaning they tend to combine with other elements. They're found naturally in a bonded state, never in a pure state.
Valence Electrons
Those electrons that occupy the outermost electron orbitals and that are involved in chemical bonding
The periodic table can also be divided into just three classes of elements, what are they?
Three classes -The metals -the nonmetals -the metalloids
What is the whole point of the periodic table?
To help predict and explain the properties of elements. These properties change as a function of the numbers of protons and electrons in the element.
What is the location of Noble Gases on the periodic table?
To the far right of the table
D-Block Elements are also know as what?
Transition Metals
What are D-Block Elements?
Transition Metals
What are mostly listed as Group B Elements?
Transition Metals
Describe Transition Metals as listed in the PowerPoint.
Transition Metals -Share properties such as conductivity, luster, malleability, atomic size, electronegativity, ionization energy, melting points, and boiling points -May have multiple oxidation states -Tend to lose electrons to become positively charged ions
We can look upon the electrons of an atom as rather peculiar apartment dwellers. Electrons prefer the floor closes to the ground and the smallest apartments. Electrons also prefer to live one to a room until each room in an apartment has one occupant. The electrons will then pair up until each room has two. Each room the apartment can hold only how many electrons?
Two
Those electrons that occupy the outermost electron orbitals and that are involved in chemical bonding
Valence Electrons
Why are valence electrons important?
Valence electrons are important because they occupy the highest energy level in the outermost shell of the atom. As a result, valence electrons are the electrons that see the most action, as in forming bonds or being gained or lost to form ions. The number of valence electrons in an atom largely determines the chemical reactivity of that atom and many other properties.
What determines whether an element is reactive or unreactive?
Valence electrons, which are involved in bonding determine whether an element if reactive or unreactive
How is an ion written?
We write an ion with its element symbol and charge
When an atom has an extra electron, what is it?
When an atom has an extra electron, it has a negative charge and is called an anion. -Oxygen commonly gains two electrons and has a negative charge.
When an atom is missing an electron, it is what?
When at atom is missing an electron, it has a positive charge and called a cation. Ex. Hydrogen commonly loses an electron and has a positive charge
When determining an element's electronic configuration, we use what?
When determining an element's electronic configuration, we use the number of electrons established by the element's atomic number.
When the element sodium, Na, loses an electron, it loses one negative charge and is left with one overall positive charge because it now has one more ____ than ___
When the element, Na, loses an electron, it loses one negative charge and is left with one overall positive charge because it now has one more proton than electron. So Na becomes Na+
Atoms have equal numbers of protons and electrons. When the number of protons equals the number of electrons, the atoms has what type of charge?
When the number of protons equals the number of electrons, the atom has a neutral charge
Atoms are at their most stable when what happens?
When their valence electrons are completely filled with electrons. Chemistry happens because atoms attempt to fill the valence shells.
Within a period, the more protons an element has, what is the correlation to electron affinity?
Within a period, the more protons an element has, the stronger its electron affinity tends to be (not perfectly smooth because other, more subtle factors are at work, but it's a good general description of what happens as you move across a period)
Group IA on the left side of the chart if often called by the family name of Alkali Metals (with the exception of hydrogen). These elements can react vigorously with water to form strong Alkaline solutions. If a friend told you that Aluminum (Al) was an Alkali Metal would he be right or wrong?
Wrong (Aluminum is located in Group IIIA and the Alkali Metals are all located in Group IA)
An electron is a particle, like a marble, but also a wave, like a beam of light. As a particle, it has a definite mass, charge, and spin, but it also has a wavelength. Is this true.
Yes
The periodic table can also be divided into just three classes of elements - the metals, the nonmetals, and the metalloids. In the periodic table, you may have noticed a steplike line. Elements to the left of this line can be classified as metals (with the exception of hydrogen). A friend informed you that the element Ti (titanium) is a metal. Is your friend correct?
Yes, Titanium can be classified as a metal.
Can you make good estimates about the relative sizes of the radii of different elements by comparing their placement in the periodic table.
Yes, you can make good estimates about the relative sizes of the radii of different elements by comparing their placement in the periodic table.
At atom's ionization energy - the energy needed to remove an outer electron - depends on the atom's size. For example, Group 1 elements have a single valence electron far away from the nucleus. These elements should have low ionization energies, is that true.
Yes. Group 1 elements - Lithium, Sodium, Potassium, Rubidium, and Cesium, the Alkali Metals shed electrons easily. In fact, they are so reactive they are never found naturally pure, but always in combination with other elements.
You can predict what kind of ion many elements will form simply by looking at what?
You can predict what kind of ion many elements will form simply by looking at their position on the periodic table. (with the exception of Row 1 (hydrogen and helium)
Effective nuclear charge
Zeff
S orbitals come in several sizes, what are they?
a 1s orbital is small, a 2s orbital is bigger, and a 3s orbital bigger still. The largest atoms in the periodic table have 7s orbitals
Strontium (Sr) is an element in the ___ family.
alkaline earth
Ba is what type
an Alkaline Earth
In addition to reactivity, another property that varies across the periodic table is what?
atomic radius, or the geometric size (not the mass) of the atoms
Is the 4s subshell filled before or after the 3d subshell?
before
What are the elements bordering the staircase?
boron, silicon, germanium, arsenic, antimony, tellurium, polonium, and astatine
The outer electrons, called valence electrons, account for most what?
chemical reactions
Shape of d orbitals?
cloverleaf shape
What orbitals have a cloverleaf shape and there are five of each sublevel. Each of these sublevels can hold 10 electrons?
d orbitals
Cation Radii Periodic Trend according to the PowerPoint?
decrease in size from their neutral atoms and know why
Shape of f orbitals
double cloverleaf shape
Shape of p orbitals?
dumbbell shape
Malleable
easy to shape
What occupies subshells
electron
What is the attraction an atom has for an added atom called?
electron affinity
Increasing numbers of protons increase the positive charge of the nucleus, which contributes to what?
electron affinity, the attraction an atom has for an added electron
What orbitals have a double cloverleaf shape and there are seven on each sublevel. Each sublevel can hold 14 electrons?
f orbitals
Allotropes
forms of an element in the same state of matter but have different physical and chemical properties (ex: diamond and graphite are both made of carbon and are both solids, they differ in their properties because they have different structures - they are isotopes)
Each shell (or floor) in the model has one or more apartments, which are called subshells. These subshells are apartments of four sizes: s, p, d, and f. An s subshell (apartment) has only a single room. A p subshell has three rooms. A d subshell has five rooms, while an f subshell has seven rooms. An s subshell will hold a maximum of two electrons according to the model. A f subshell will hold a maximum of how many electrons
fourteen (7 rooms x 2 electrons/room)
Iodine (I) is an element in the ___ family
halogen
Nonmetals are located on the right side of the steplike line of the periodic table. Which of the following families of elements are classified as nonmetansl? (halogens, alkaline earths, noble gases)
halogens and noble gases
Shellf 4 has what that holds up to 32 electrons total
have all of that plus 7 f orbitals
What are the properties of metalloids?
have properties between those of metals and nonmetals
Anion Radii Periodic Trend according to the PowerPoint?
increase in size from their neutral atoms and know why
Describe nonmetals
inert extremely unreactive
What two series on the periodic table have an added wrinkle
lanthanides and actinides
A substance that shines and conducts heat and electricity is a (metal, nonmetal, metalloid)
metal
Identify as a property of metal or nonmetal shiny
metal
Identify as a property of metal or nonmetal Ductile (easy to stretch into wires)
metals
Identify as a property of metal or nonmetal Reactive with nonmetals
metals
Identify as a property of metal or nonmetal high density
metals
Identify as a property of metal or nonmetal high melting point and boiling point
metals
Identify as a property of metal or nonmetal shiny
metals
The periodic table can also be divided into just three classes of elements - the metals, the nonmetals, and the metalloids. In the periodic table, you may have noticed a steplike line. Elements to the left of this line can be classified as what (with the exception of hydrogen)
metals
Elements to the left of of the staircase on the period table are what?
metals (except hydrogen in Group 1A)
What are the most extreme nonmetals
noble gases
An unknown element is a solid but does not conduct electricity. The element is probably a (metal, nonmetal)
nonmetal (some nonmetals are solid, although most are gases at room temperature. Nonmetals do not conduct electricity well, but metals usually do)
An unknown element exists as a gas at room temperature. How would you classify the unknown element, as a metal or as a nonmetal?
nonmetal (with the exception of mercury, which is liquid at room temperature, all metals are solid at ordinary room temperature)
Nonmetals have properties almost opposite those of metals. Nonmetals are usually very brittle and do not conduct electricity or heat well. Most nonmetals are gases at ordinary temperatures, although some are liquids or solids. An unknown element exists as a gas at room temperature. How would you classify the unknown element, as a metal or a nonmetal?
nonmetal (with the exception of mercury, which is liquid at room temperature, all metals are solid at ordinary room temperature)
A third category of elements is classified as metalloids because they don't clearly fall into either the metal or nonmetal categories. Metalloids border the steplike line on the periodic table and include elements such as Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Born (B), Tellurium (Te), Polonium (Po), and Astatine (At). Metalloids could be expected to have some of the properties of metals and some of the properties of ___
nonmetals
Elements to the right of the staircase are what?
nonmetals
Identify as a property of metal or nonmetal Reactive with metals (except for last group)
nonmetals
Identify as a property of metal or nonmetal brittle when solid
nonmetals
Identify as a property of metal or nonmetal dull-looking
nonmetals
Identify as a property of metal or nonmetal often liquid or gaseous at room temperature
nonmetals
Identify as a property of metal or nonmetal poor electrical conductivity
nonmetals
The electron configurations within each energy level are called what?
orbitals
What orbitals have a dumbbell shape and there are 3 orbitals on each p sublevel, so each p sublevel can hold 6 electrons?
p orbitals
What is the outermost subshell electron configruation common to all the halogens?
p5
Shell 1 has only a what: which is spherical. It can hold one or two electrons.
s orbital
What orbitals have a spherical shape and can hold 2 electrons each
s orbitals
Name three common kinds of orbitals, each with its own shape and special properties.
s orbitals, p orbitals, and d orbitals (there are also f and g orbitals)
There are four know orbital shapes - what are they?
s, p, d, and f
There are four types of orbitals, what are they?
s, p, d, and f
The floors in the apartment building are called shells in the electron model and are numbered 1 through 7. We learned that electrons prefer the floor closes to the ground and the smallest apartments. What shell will be occupied first by the electrons?
shell 1 (the first floor)
Each group of elements in the periodic table has similar subshells with similar number of electrons in the outermost shell. The outermost shell consists of the subshells that are filled last. This situation serves to explain the (similar, greatly different) ___ chemical properties of elements within the same groups
similar chemical properties of elements within the same groups
Each shell (or floor) in the model has one or more apartments, which are called subshells. These subshells are apartments of four sizes: s, p, d, and f. An s subshell (apartment) has only a single room. A p subshell has three rooms. A d subshell has five rooms, while an f subshell has seven rooms. An s subshell will hold a maximum of two electrons according to the model. A p subshell will hold a maximum of how many electrons?
six (3 rooms x 2 electrons/room)
Shape of s orbitals?
spherical shape
Periodic trends smaller distance equals what?
stronger attraction
Periodic trends stronger magnet equals what?
stronger attraction
Each shell (or floor) in the model has one or more apartments, which are called subshells. These subshells are apartments of four sizes: s, p, d, and f. An s subshell (apartment) has only a single room. A p subshell has three rooms. A d subshell has five rooms, while an f subshell has seven rooms. An s subshell will hold a maximum of two electrons according to the model. A d subshell will hold a maximum of how many electrons?
ten (5 rooms x 2 electrons/room)
Describe metals?
tend to be solid and shiny to conduct electricity and heat to give up electrons to be malleable (easily shaped) to be ductile (easily drawn out into wire)
Atoms tend to take the shortest path to a complete octet, whether that means ditching a few electrons to achieve a full octet at a lower energy level or grabbing extra electrons to complete the octet at their current energy level. In general, nonmetals on the right side of the periodic table tend to _____ electrons?
tend to gain electrons
You can predict how many electrons an atom will gain or lose to become an ion. Group VA elements gain or lose how many electrons?
tend to gain three electrons
You can predict how many electrons an atom will gain or lose to become an ion. Group VIA elements gain or lose how many electrons?
tend to gain two electrons
Atoms tend to take the shortest path to a complete octet, whether that means ditching a few electrons to achieve a full octet at a lower energy level or grabbing extra electrons to complete the octet at their current energy level. In general, metals on the left side of the periodic table (an in the middle) tend to _____ electrons?
tend to lose electrons
What is electron affinity?
the attraction an atom has for an added electron
What is the periodic law?
the physical and chemical properties of the elements are periodic functions of their atomic numbers
In making gold leaf, we are using what common property of metals?
the property of malleability
Another word for the outermost electrons in an atom, particularly in the s and p orbitals is what?
valence electrons Note: Valence electrons in the s and p orbitals play an important role in chemical bonding
Elements within any group have what?
very similar properties
Another way to represent the arrangement of electrons around an atom is to use arrows as electrons and boxes to represent orbitals. The boxes become occupied by electrons as we "build up" the atoms of each element in the periodic table. Remember, only one electron will occupy an orbital in a given subshell until all the orbitals in that subshell have one electron in them. Then and only then will a second electron occupy each orbital. Using this method, the electron arrangement for ₁₂Mg follows. Pretend a box is around each set of up down arrow or if in only one direction around it in singular 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ The arrow notation for ₇N is 1s↑↓ 2s↑↓ 2p↑↑↑ Note the unpaired or single electrons in the partially filled 2p subshell. The electrons occupy as many orbitals as possible in the same subshell before pairing with another electron. This is known as the Principle of Maximum Multiplicity. Using the Principle of Maximum Multiplicity and the arrow notation, indicate the arrangement of electrons for the following ₁₄Si
₁₄Si 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ 3p ↑↑
Another way to represent the arrangement of electrons around an atom is to use arrows as electrons and boxes to represent orbitals. The boxes become occupied by electrons as we "build up" the atoms of each element in the periodic table. Remember, only one electron will occupy an orbital in a given subshell until all the orbitals in that subshell have one electron in them. Then and only then will a second electron occupy each orbital. Using this method, the electron arrangement for ₁₂Mg follows. Pretend a box is around each set of up down arrow or if in only one direction around it in singular 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ The arrow notation for ₇N is 1s↑↓ 2s↑↓ 2p↑↑↑ Note the unpaired or single electrons in the partially filled 2p subshell. The electrons occupy as many orbitals as possible in the same subshell before pairing with another electron. This is known as the Principle of Maximum Multiplicity. Using the Principle of Maximum Multiplicity and the arrow notation, indicate the arrangement of electrons for the following ₁₆S
₁₆S 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ 3p ↑↓↑↑
Another way to represent the arrangement of electrons around an atom is to use arrows as electrons and boxes to represent orbitals. The boxes become occupied by electrons as we "build up" the atoms of each element in the periodic table. Remember, only one electron will occupy an orbital in a given subshell until all the orbitals in that subshell have one electron in them. Then and only then will a second electron occupy each orbital. Using this method, the electron arrangement for ₁₂Mg follows. Pretend a box is around each set of up down arrow or if in only one direction around it in singular 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ The arrow notation for ₇N is 1s↑↓ 2s↑↓ 2p↑↑↑ Note the unpaired or single electrons in the partially filled 2p subshell. The electrons occupy as many orbitals as possible in the same subshell before pairing with another electron. This is known as the Principle of Maximum Multiplicity. Using the Principle of Maximum Multiplicity and the arrow notation, indicate the arrangement of electrons for the following ₂₃V
₂₃V 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ 3p ↑↓↑↓↑↓ 4s↑↓ 3d↑↑↑
How would you write the box and arrow notation for ₂₅Mn?
₂₅Mn 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ 3p ↑↓↑↓↑↓ 4s↑↓ 3d↑↑↑↑↑
Another way to represent the arrangement of electrons around an atom is to use arrows as electrons and boxes to represent orbitals. The boxes become occupied by electrons as we "build up" the atoms of each element in the periodic table. Remember, only one electron will occupy an orbital in a given subshell until all the orbitals in that subshell have one electron in them. Then and only then will a second electron occupy each orbital. Using this method, the electron arrangement for ₁₂Mg follows. Pretend a box is around each set of up down arrow or if in only one direction around it in singular 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ The arrow notation for ₇N is 1s↑↓ 2s↑↓ 2p↑↑↑ Note the unpaired or single electrons in the partially filled 2p subshell. The electrons occupy as many orbitals as possible in the same subshell before pairing with another electron. This is known as the Principle of Maximum Multiplicity. Using the Principle of Maximum Multiplicity and the arrow notation, indicate the arrangement of electrons for the following ₂₆Fe
₂₆Fe 1s↑↓ 2s↑↓ 2p↑↓↑↓↑↓ 3s↑↓ 3p ↑↓↑↓↑↓ 4s↑↓ 3d↑↓↑↑↑↑
Electron Configuration for Example: ₈₆Rn Write down and then check
₈₆Rn 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s² 4f¹⁴5d¹⁰6p⁶
Single-atom anions are named by adding what to the root of their elemental name?
"IDE" Examples: Fluoride, Oxide, etc
Cations have superscripts with what type of sign?
+ positive
Anions have superscripts with what type of sign?
- or negative
What are the 6 groups of P-Block Elements?
-Boron Family -Carbon Family -Nitrogen Family -Oxygen Family -The Halogens -The Noble Gases (Note: Helium is part of S Block) (Not Verified by Two Sources; PowerPoint says 6 but lists 5)
Metals have a lustrous or shiny surface and are solid and ordinary room temperature (with the exception of mercury, which is liquid at room temperature). Metal cooking utensils take advantage of what two properties of metal? (conduct electricity, conducts heat, ductile, solid)
-Conducts Heat -And is Solid
What are two main principles of Coulombic Attraction?
-Greater charge equals stronger attraction -Smaller distance equals greater attraction
Describe the properties of Alkaline Earth Metals as listed in the PowerPoint?
-Harder than Alkali Metals -Although less abundant, still found as compounds in the Earth's crust -Contains 2 valence electrons
Describe Transition Metals
-May have multiple oxidation states -Tend to lose electrons to become positively charged ions
Describe the properties of Alkali Metals as described in the PowerPoint?
-Soft enough to cut with a knife -Extremely reactive, found as compounds in nature, stored in oil in labs to prevent reacting with oxygen -Contains 1 valence electron
Besides being malleable, metals are also good conductors of heat and electricity. Copper is useful in making electrical wiring. What two metallic properties would be useful in electrical wiring?
-The metal is a conductor of electricity -And it is ductile (can be drawn into fine wires)
The first shell (floor) has only one subshell (apartment), which is an s subshell. Because of the location on the first shell, it is called a 1s subshell. How many orbitals (rooms) are there in this 1s subshell?
1 (s subshells have only 1 orbital)
There are how many orbitals in each s sublevel?
1 orbital
Shell 2 has what, which look something like dumbbells, when full, this shell holds eight electrons
1 s and 3 p orbitals
Shell 3 has what that when full holds 18 electrons
1 s, 3 p and 5 d orbitals
Which atom is larger, Na or K (CER)
1+1+1=3 Potassium is larger Potassium has one more principal energy level than Sodium. The more energy levels, the farther away from the nucleus the valence electrons are, creating less of an attraction to the nucleus and a bigger atom.
The d orbitals have a cloverleaf shape and there are five on each d sublevel. Each d sublevel can hold how many electrons?
10
The f orbitals have a double cloverleaf shape and there are seven on each f sublevel. Each f sublevel can hold how many electrons?
14
Let's review what we have just learned. Assume that we have only seven floors in our "building." A subshell may hold as many as ___ electrons or as few as ___ electron(s), assuming full occupancy.
14, 2
How many orbitals are there in the fourth shell?
16 (1 s orbital, 3 p orbitals, 5 d orbitals, and 7 f orbitals)
What Group Number are Halogens in the P-Block Elements according to the PowerPoint?
17
What Group Number are Noble Gases in the P-Block Elements according to the PowerPoint?
18
The third shell has three subshells: s, p, and d. How many electrons can be in the third shell?
18 (9 orbitals x 2 electrons/orbital)
Which subshell is filled first?
1s
Electrons fill orbitals with the lowest energy first. The sequence from lowest to highest energy is what?
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
What is Lithium's electronic configuration?
1s², 2s¹ Note: As each shell is filled, the next electron moves to the next closest orbital.
What is Helium's electronic configuration?
1s². Note: the first s orbital is filled first.
The following notation is used to indicate the number of electrons in each subshell of an atom. For example, neon has ten electrons, therefore its subshells are written as 1s²2s²2p⁶. The numbers to the upper right of each subshell indicate the number of electrons in each subshell. If we add these numbers (2+2+6=10) we get the number of electrons in a neon atom. How would you use this notation for Magnesium (Mg) atom?
1s²2s²2p⁶3s² (2+2+6+2=12)
What is hydrogen's electronic configuration?
1s¹
Each orbital can hold up to how many electrons?
2
The first shell (floor) has only one subshell (apartment), which is an s subshell. Because of the location on the first shell, it is called a 1s subshell. How many electrons will the subshell hold?
2 (each orbital holds only 2 electrons)
The second shell (floor) only has an s subshell (apartment) and a p subshell. How many subshells are in the second shell?
2 (s an dp)
For Alkaline Earth Metals, the subshell of the outermost shell in each alkaline earth is made up of ___ electrons in a(n) ___ subshell.
2 electrons in a s subshell
The second shell (floor) only has an s subshell (apartment) and a p subshell. If the s subshell is called 2s, what do you suppose the p subshell is called?
2p
2s means what?
2s means the s orbital in shell 2
The third shell has three subshells: s, p, and d. How many subshells are in the third shell?
3
Which has a higher first ionization energy. Li or Na (CER)
3 AL has a higher EA AL has a higher Zeff The higher Zeff, the easier to hold an electron in the outer shell (EA)
Which is larger, Br or Br- (CER)
3 Br- is larger Br- has one more electron than Br With an extra electron, the electrons repel each other more, creating a larger atom
Which is larger, Na or Na+ (CER)
3 Na is larger Na has one more energy level than Na+ and has a lower Zeff The more energy levels, the farther away from the nucleus the valence electrons are, creating less of an attraction to the nucleus and a bigger atom. The lower Zeff, the less the nucleus pulls in valence electrons, creating an attraction to the nucleus and a bigger atom.
Which atom is larger, Na or Al(CER)
3 Sodium is larger Na has a weaker Zeff also FCA than AL The weaker Zeff, the less the nucleus pulls in valence electrons, creating a bigger atom
The second shell (floor) only has an s subshell (apartment) and a p subshell. How many orbitals (rooms) are in that p subshell?
3 (P subshells have 3 orbitals)
There are how many orbitals in each p sublevel?
3 orbitals
How many electrons with the fourth shell hold?
32 (16 orbitals x 2 electrons/orbital)
Let's review what we have just learned. Assume that we have only seven floors in our "building." A shall may hold as many as ___ electrons or as few as ___ electrons, assuming full occupancy
32, 2
The 4s orbitals fills as we begin the fourth row of the table. Next, electrons begin to occupy the what orbitals?
3d
The third shell has three subshells: s, p, and d. What are they called?
3s, 3p, 3d
How many subshells are in the seventh shell?
4
How many subshells are there in the fifth shell?
4
The second shell (floor) only has an s subshell (apartment) and a p subshell. How many orbitals are there in the second shell?
4 (1 s orbital and 3 p orbitals)
Let's review what we have just learned. Assume that we have only seven floors in our "building." A shell may have as many as ___ subshells or as few as ___ subshells
4, 1
4d means what?
4d means the d orbital in shell 4 Note each arrow leads to the orbital with the next-highest energy.
Shells 4 through 7 each have four subshells: s, p, d, and f. What would you call the subshells on the fourth shell?
4s, 4p, 4d, 4f
Rank the following in order of decreasing ionization energy: Si, Ga, O, Ba
5 O, Si, Ga, Ba O has higher Zeff and less energy level than Si Si has higher Zeff and 1 less energy level than Ga Ga has higher Zeff and 2 less energy levels than Ba As Zeff increases and energy levels decrease, inonization energy increases
Rank the following in order of increasing atomic radius: Te, Sr, Ca, S (CER)
5 S, Ca, Te, Sr S has 1 less energy and higher Zeff than Ca Ca has less energy levels than TE Te has higher Zeff than S As energy levels increase, atomic radius increases. As Zeff decreases, atomic radius increases
The incomplete subshell in each halogen is made up of how many electrons? In what subshell?
5 electrons in p subshell
There are how many orbitals in each d sublevel?
5 orbitals
The p orbitals have a dumbbell shape and there are 3 orbitals on each p sublevel, so each p sublevel can hold how many electrons?
6
Shells 4 through 7 each have four subshells: s, p, d, and f. What would you call the subshells on the sixth shell?
6s, 6p, 6d, 6f
There are how many orbitals in each f sublevel?
7 orbitals
Let's review what we have just learned. Assume that we have only seven floors in our "building." A subshell may have as many as ___ orbitals or as few as ___ orbitals
7, 1
Apartment buildings may have several floors. The model we discuss has several floors, but only the first how many floors will be occupied?
7. All the electrons of the elements known today will fit within seven floors of the building. Additional floors are available but will only be occupied in special cases.
The second shell (floor) only has an s subshell (apartment) and a p subshell. How many electrons can occupy the second shell?
8 (4 orbitals x 2 electrons/orbital)
All main group elements are most stable (think "Happiest") with a full shell of how many valence electrons?
8 valence electrons
The third shell has three subshells: s, p, and d. How many orbitals are in the third shell?
9 (1 s orbital, 3 p orbitals, 5 d orbitals
The subshell of greatest energy of each noble gas is (mark the correct answer): ___a completely filled with electrons ___b half-filled with electrons ___c can take one more electron each
A completely filled with electrons Only six electrons can occupy the orbitals in a p subshell
Each room in a subshell is called an orbital. We know then that an s subshell will consists of one orbital with a capacity (occupancy) of two electrons. A d subshell will consists of ___ orbitals with a total capacity of ___ electrons
A d subshell will consists of ___ orbitals with a total capacity of ___ electrons 5, 10
Cl is what type
A halogen
What is the different between a hydrogen atom and a hydrogen ion?
A hydrogen atom has 1 proton and 1 electron with a neutral charge; a hydrogen ion has 1 proton and 0 electrons and has a positive charge
Each room in a subshell is called an orbital. We know then that an s subshell will consists of one orbital with a capacity (occupancy) of two electrons. A p subshell will consists of three orbitals with a total subshell capacity of ___ electrons
A p subshell will consists of three orbitals with a total subshell capacity of 6 electrons
When a highly electropositive atom meets a highly electronegative one, the result is an ionic bond. The electropositive atom easily gives away one or more electrons and becomes what?
A positively charge cation
What series in F-Block Elements have most of them as synthetic elements that are created in particle accelerators?
Actinide Series
What series in F-Block elements are radioactive elements?
Actinide Series
What series in F-Flock Elements have only four that exist in nature?
Actinide Series
Describe the Actinide Series according to the PowerPoint
Actinide Series -Radioactive elements -Only four exist in nature; the rest are synthetic elements that are created in particle accelerators
After filling the s orbital, electrons begin to fill what?
After filling the s orbital, electrons begin to fill the p orbitals (Note: According to Hund's rule, p, d, and f orbitals in a sublevel has to each be filled with a single electron before a second electron can pair in any orbital.)
An unknown element is placed in water. A vigorous reaction takes place, and the result is an alkaline solution. Of which family is the element probably a member? (alkaline earth, alkali metal, noble gas)
Alkali Metal (Alkali Metals react directly with water to form alkaline solutions. The oxides of alkaline earth elements react with water to form alkaline solutions)
Group IIA elements are know as the Alkaline Earth Metals because the oxides of these metals (chemical compounds of the metals and oxygen) form alkaline solutions in water. The element potassium (K) can be classified as a(n) (noble gas, alkaline earth, alkali metal)
Alkali Metal (Group IA)
Group 1A is also known as what?
Alkali Metals
What is Group 1 Called
Alkali Metals
What is Group 1 called according to the PowerPoint?
Alkali Metals
What group is so reactive that they are never found naturally pure but always found in combination with other elements?
Alkali Metals Note: in pure form, they can be explosively dangerous
The element Ba (Barium) can be classified as a(n) (alkali metal, alkaline earth, noble gas)
Alkaline Earth (Group IA)
Group IIA on the Periodic Table is called what?
Alkaline Earth Metals
What is Group 2 Called
Alkaline Earth Metals
What is Group 2 called according to the PowerPoint?
Alkaline Earth Metals
Forms of an element in the same state of matter but have different physical and chemical properties
Allotrope
Forms of an element in the same state of matter but have different physical and chemical properties.
Allotropes
Electronic configuration of Aluminum, AL
Aluminum, AL Ne3s²3p¹ After 2p fills up, the lowest-energy orbital is 3s, in the third shell, followed by 3p
What element has the electron configuration 1s²2s²2p⁶3s²3p¹? And in what group would it be found in the periodic table
Aluminum; Group IIIA
Na is what type
An Alkali metal
What is the difference between an Oxygen atom and an Oxygen ion?
An Oxygen atom has 8 protons and 8 electrons and has a neutral charge. An Oxygen ion has 8 protons and 10 electrons and has a negative charge
Ion
An atom or group of elements that bears a positive or negative charge
The energy needed to remove an outer electron
An atom's ionization energy
Each room in a subshell is called an orbital. We know then that an s subshell will consists of one orbital with a capacity (occupancy) of two electrons. An f subshell will have ___ orbitals and hold ___ electrons
An f subshell will have ___ orbitals and hold ___ electrons 7, 14
When a highly electropositive atom meets a highly electronegative one, the result is what?
An ionic bond
When a highly electropositive atom meets a highly electronegative one, the result is an ionic bond. The electronegative atom loves to acquire extra electrons and in doing so becomes what?
Anion
Atoms that gain electrons (like nonmetals) acquire negative charge becoming what?
Anions
Negative Ions
Anions
You have just learned the notation a chemist uses to indicate the arrangement of electrons in an atom. This arrangement is called its electron configuration. Determine the electron configuration of Argon ₁₈Ar
Argon 1s²2s²2p⁶3s²3p⁶
What is the most common of the noble gases?
Argon (almost 1 percent of the atmosphere). Is used in ordinary incandescent light bulbs, since it won't react with the hot filament.
Electronic configuration of Argon
Argon, AR Ne3s²3p⁶ After 2p fills up, the lowest-energy orbital is 3s, in the third shell, followed by 3p
Moseley
Arranged atoms according to increasing atomic number
Tell me about Moseley and the Periodic Table according to the PowerPoint.
Arranged atoms according to increasing atomic number -Gave us the periodic law - the physical and chemical properties of the elements are periodic functions of their atomic numbers -Produced a table in which elements with similar properties fell into the same column, or group
Tell me about Mendeleev and the Periodic Table according to the PowerPoint
Arranged the elements in order of increasing atomic mass -Created a table in which element with similar properties were grouped together -In this way, properties of undiscovered elements could be predicted -Did not apply to some elements
How was Mendeleev's arrangement useful?
Arranged the elements in order of increasing atomic mass (elements with similar properties were grouped together). In this way, properties of undiscovered elements could be predicted. (Did not apply to some elements)
Mendeleev
Arranged the elements in order of increasing atomic mass; Created a table in which elements with similar properties were grouped together. In this way, properties of undiscovered elements could be predicted.
What are the electron configurations of the following elements? Arsenic (As)
Arsenic (As) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p³
As we build up an atom, each electron "wants" to go into what type of energy state?
As we build up an atom, each electron "wants" to go into the lowest available energy state. We start at the lowest, then when that fills up, go to the next-lowest, etc.
As we have mentioned previously, electrons prefer the lower shells (floors) and the smaller subshells (apartments). Electrons prefer the smaller subshells to such a degree that they will sometimes occupy a smaller subshell on the next higher shell rather than the larger subshell on the lower shell. By experimentation, it has been determined that electrons will fill the 1s subshell (apartment) first. They will then fill the 2s subshell, and then the 2p subshell. Next, they will fill the 3s subshell. However, before going into the large five orbital 3d subshell, electrons will first fill the 4s subshell. After filling the 4s subshell, electrons will then proceed to fill the 3d subshell. The 4p subshell is filled next. The 4d is filled after 5s. Next the electrons fill the 5p subshell. Then the small 6s subshell is filled. The very large 4f subshell is occupied only after 6s is filled. After 4f comes 5d. Next is 6p, then 7s, and then 5f. Note that as we fill consecutive subshells, the energy of the electrons does what?
As we fill the consecutive subshells, the energy of the electrons increases. Electrons in the 2s subshell have higher energy than electrons in the 1s subshell; 2p electrons have a higher energy than 2s electrons, and so on.
As you move down or to the right on the periodic table, elements have both more what and what
As you move down or to the right on the periodic table, elements have both more protons and more electrons (However as you move down the periodic table do the added electrons occupy higher energy levels)
One-half the distance between the nuclei of identical atoms that are bonded together.
Atomic Radii
The geometric size (not the mass) of the atoms
Atomic Radius
Why does the atomic radius tend to decrease as you move to the right of the periodic table?
Atomic radius tends to decrease as you move to the right, because the increasing positive charge of the nuclei pulls the electrons of that energy level inward.
Atomic size moving down a column, what happens to atoms?
Atomic size moving down a column, they get bigger
Anions
Atoms that gain electrons (like nonmetals) acquire negative charge, becoming anions, such as CL- or O2- (2 is written up top)
Cations
Atoms that lose electrons (like metals) acquire positive charge, becoming cations such as NA+ or Mg2+ (2 is above the g)
Atoms toward the right side of the periodic table tend to have what type of electron affinity?
Atoms toward the right side of the periodic table tend to have higher electron affinity: small diameter (so electrons can get closer), big pull from the nucleus, and an unfilled orbital or two (except in the last group - they're full)
What happens to attraction with Zeff when Zeff is greater?
Attraction is ↑
Which has a larger atomic radius, silicon or barium?
Barium's atomic radius is larger. Atomic size tends to increase from top to bottom and from right to left. Barium (Ba) is farther down and to the left on the periodic table than Silicon (Si). Barium has more energy levels and is therefore larger.
What type of ion is Beryllium most likely to form?
Be2+ (2 is superscript), also known as the beryllium cation. By losing two electrons, beryllium, which is in Group IIA, assumes a full octet valence shell, with two electrons like helium.
As you move down the periodic table, why does the atomic radius tend to increase?
Because even though you're adding positively charged protons to the nucleus, you're now adding electrons to higher and higher energy levels, which correspond to larger and larger electron shells
Why do elements within a group tend to have similar chemical properties?
Because they have similar arrangements of electrons at their outermost borders or shells. As you move across a period, however, the properties of the elements tend to change gradually. By the time you reach the right edge of the periodic table, the elements' outermost shells are completely full. With full outer shells, the elements are stable and have no drive to react.
Why are Halogens in Group VIIA so reactive?
Because they need only to acquire on electron to have a completely filled valence shell.
Why are Alkali metals in Group IA so reactive?
Because they need only to give up one electron to have a completely filled valence shell
Why are noble gases called what they are?
Because they seem to consider themselves above the other elements. They're very unreactive and rarely bond to form compounds.
Electronic configuration for Beryllium
Berryllium 1s²2s² Beryllium, Be, completes the 2s orbital
This group in P-Block Elements if always found combined with other elements in nature according to the PowerPoint?
Boron
Describe the Boron Group or Family in P-Block according to the PowerPoint?
Boron -Group 13 -Always found combined with other elements in nature -Contains 3 valence electrons
Electronic configuration for Boron
Boron 1s²2s²2p¹ Boron, B, add an electron to a 2p orbital
How many electrons will be gained or lost by Boron when forming an ion?
Boron (B) loses three electrons for form the boron cation B3+ (3 is superscript)
Group 13 in P-Block Elements refer to what according to PowerPoint?
Boron Group or Family
Group in P-Block Elements that have 3 valence electrons according to the PowerPoint?
Boron Group; Group 13
How many valence electrons does Calcium (Ca) have?
Calcium (Ca) have two valence electrons because it's in Group IIA
Describe the Carbon Group or Family in P-Block according to the PowerPoint?
Carbon -Group 14 -Group varies in many properties because? -Contains 4 valence electrons -Allotropes - forms of an element in the same state of matter but have different physical and chemical properties
Electronic configuration for Carbon
Carbon 1s²2s²2p² Carbon, C, adds an electron to the second p orbital
Group 14 in P-Block Elements refer to what according to PowerPoint?
Carbon Group or Family
Group in P-Block Elements that have 4 valence electrons according to the PowerPoint?
Carbon Group; Group 14
Ionic Radii Period Trend according to the PowerPoint?
Cation radii: decrease in size from their neutral atoms Anion radii: increase in size from their neutral atoms And know why
Atoms that lose electrons (like metals) acquire positive charge becoming what?
Cations
Positive Ions
Cations
The "glue" that holds molecules together
Chemical Bonding
The elements within a group have widely varying numbers of protons, neutrons, and electrons. Why, then, do elements in a group tend to have similar chemical properties?
Chemical properties come mostly from the arrangement of electrons in the outermost shell of an atom. Although the elements at the top and bottom of a give group (like fluorine and astatine, for example) have very different numbers of protons, neutrons, and electrons, the arrangements of electrons in their outermost shells are very similar.
What is chemistry really about as it relates to this chapter?
Chemistry is really about the making and breaking of bonds, valence electrons are the most important particles for chemistry
How many electrons will be gained or lost by Chlorine when forming an ion?
Chlorine (Cl) gains one electron to form the chloride anion Cl-
Electronic configuration of Chlorine
Chlorine, CL Ne3s²3p⁵ After 2p fills up, the lowest-energy orbital is 3s, in the third shell, followed by 3p
Cobalt's atomic number is 27. File in the blanks to find Cobalt's electronic configuration. 1s², ___, 2p⁶, 3s², ___, 4s², 3d⁷
Cobalt's electronic configuration Blanks 2s² and 3d¹⁰ 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d⁷ Note: This is because Cobalt only has 7 electrons in its outer shell, even though d orbitals can hold up to 10 electrons
Elements with similar properties fall into the same what according to the PowerPoint?
Column or Group
What is salt?
Combination of a metal and a halogen
Atoms are the most stable when their valence shells are what?
Completed filled with electrons
What are the properties of Alkaline Earth Metals?
Contain 2 valence electrons; P-block elements 6 groups
What is the physical "law" that mathematically describes the force of attraction between two ions
Coulomb's Law
What describes the attraction between two charged particles?
Coulombic Attraction
D sublevels can hold how many electrons each?
D sublevels can hold 10 electrons each.
Transition metals are part of what block of elements according to the PowerPoint?
D-Block
Electron Affinity Group Tend according to the PowerPoint?
Decreases down a group and know why
Electronegativity Group Tend according to the PowerPoint?
Decreases down a group and know why
Ionization Energy Group Tend according to the PowerPoint?
Decreases down a group and know why
The properties of elements emerge mostly from their different numbers of what?
Different numbers of protons and electrons and from the arrangement of their electrons
Why have the two series Lanthanides and Actinides lifted out of regular order and placed below the rest of the table?
Doing so prevents the table from being inconveniently wide The lanthanides all have pretty similar properties, as do the lactinides
Easy to stretch into wries
Ductile
Each electron in an atom is in a little cloud called a what which can hold up to two electrons?
Each electron in an atom is in a little cloud called an orbital which can hold up to two electrons, and the overall electron cloud of an atom is built up from these orbitals.
Ductile
Easy to stretch into wires
Measures an atom's "willingness" to become an anion i.e. to add an extra electron
Electron Affinity
The difference in energy when an electron is added to a neutral atom.
Electron Affinity
What is the flip side of ionization energy
Electron Affinity
An orbiting electron may absorb a jolt of energy too, but the electron must jump to an orbit consists with what?
Electron must jump to an orbit consistent with a whole number of wavelengths.
Nonmetals tend to accept extra electrons. Some nonmetals, like Fluorine and Oxygen, avidly grab electrons, while others, such as carbon can take them or leave them. This is called what?
Electronegative
The ability of an atom in a compound to attract electrons from another atom in the compound.
Electronegativity
Complete the following electronic configuration: Oxygen ___, 2s², 2p⁴
Electronic Configuration Oxygen Blank 1s² 1s², 2s², 2p⁴
Complete the following electronic configuration: Phosphorus 1s², ___, 2p⁶, 3s², ___
Electronic Configuration Phosphorus Blanks 2s² and 3p³ 1s², 2s², 2p⁶, 3s², 3p³
Complete the following electronic configuration: Strontium 1s², 2s², ___, ___, 3p⁶, 4s², ___, 4p⁶, ___
Electronic Configuration Strontium Blanks 2p⁶, 3s², 3d¹⁰, 5s² 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s²
Electron affinity increases as you move in what direction on the periodic table?
Electronic affinity increases as you move up and to the right of the periodic table
Electrons can absorb only certain what just enough to jump the electron to one of the higher available orbits
Electrons can absorb only fixed amounts of energy, just enough to jump the electron to one of the higher available orbits.
Electrons fill orbitals with the what type of energy first.
Electrons fill orbitals with the lowest energy first.
Electrons in the highest energy level occupy what shell of the atom?
Electrons in the highest energy level occupy the outermost shell of the atom and are called valence electrons
Electrons orbit around what?
Electrons orbit around the nucleus of at atom. The nucleus is where the protons and neutrons are, in the center of the atom.
Metals tend to give up electrons, though some metals do so more enthusiastically than others. A chemist would say that metals are more or less what?
Electropositive
Ions
Elements are so insistent about having filled valence shells that they'll gain or lose valence electrons to do so. Atoms that gain or lose electrons in this way are called ions.
In Moseley's arrangements elements that fell into the same column, or group - describe it.
Elements with similar properties fell into the same column, or group.
Chromium has more electrons than scandium. Why, then does scandium have a large atomic radius?
Even though Chromium (Cr) has more electrons than Scandium (Sc), those extra electrons occupy the same energy level, because the two elements are in the same row on the periodic table. Furthermore, Chromium has more protons than Scandium (as you can tell by Chromium's position to the right of Scandium), creating a more positively charged nucleus that pulls the electrons of a given energy level inward, thereby decreasing the atomic radius
Give an example of an Allotrope.
Example: Diamond and graphite are both made of carbon and are both solids, they differ in their properties because they have different structures - they are isotopes
F sublevels can hold how many electrons each?
F sublevels can hold up to 14 electrons each
The Lanthanide Series and the Actinide Series are part of what block of elements according to the PowerPoint?
F-Block
Force of Attraction Formula
F=K*Q₁*Q₂/D²
What is the most Electronegative Atom?
Fluorine
Fluorine and sodium are only two atomic numbers apart on the periodic table. Why, then, does fluorine form an anion, F-, whereas sodium forms a cation, Na+?
Fluorine Fluorine (F) is in Group VIIA, just one group to the left of the noble gases, and therefore needs to gain only one electron to complete a valence octet. Sodium Sodium (Na) lies just one group to the right of the noble gases, having wrapped around into Group IA of the next energy level. Therefore, Sodium needs to lose one electron to achieve a full valence octet.
Electronic configuration for Fluorine
Fluorine, F 1s²2s²2p⁵
Allotrope
Forms of an element in the same state of matter but have different physical and chemical properties
Alkali Metals are found naturally in what state
Found naturally in a bonded state, never in a pure state
Octet
Full shell of eight valence electrons
You can predict how many electrons an atom will gain or lose to become an ion. Group VIIA (Halogen) elements gain or lose how many electrons?
Gain one electron
How many valence electrons does Germanium (Ge) have?
Germanium (Ge) has four valence electrons because it's in Group IVA
Atomic size going along a row from left to right, what happens to atoms
Going along a row from left to right, atoms get smaller
Atomic Radii Periodic Trend according to the PowerPoint?
Gradual decrease in atomic radii from left to right and know why
Atomic Radii Group Trend according to the PowerPoint?
Gradual increase down a group and why
Gives the names of several Allotropes of Carbon according to the PowerPoint?
Graphite Diamond BC8 Fullerene Nanotube Graphene
The elements in Group VIIA are known as halogens, which means "salt formers." Elements from the halogen family combine with metals to form compounds known as salts. Common table salt (NaCl) is made up of sodium(Na) and chlorine (Cl). These two elements (Na and Cl) are members of which families or groups. What about Na.
Gropu IA, the alkali metals (either answer is acceptable)
What are the two groups of S-Block elements according to the PowerPoint?
Group 1 - Alkali Metals Group 2 - Alkaline Earth Metals
What group number is Boron in P-Block Elements as listed in the PowerPoint?
Group 13
What group number is Carbon in P-Block Elements as listed in the PowerPoint?
Group 14
F-Block Elements have similar reactivity to what group?
Group 2 which is Alkaline Earth Metals
The elements in Group VIIA are known as halogens, which means "salt formers." Elements from the halogen family combine with metals to form compounds known as salts. Common table salt (NaCl) is made up of sodium(Na) and chlorine (Cl). These two elements (Na and Cl) are members of which families or groups. What about Cl.
Group VIIA, the halogens (either answer is acceptable)
The columns in the periodic table are called
Groups or Families
The next-to-last group is especially electron hungry. These elements are called what and have a small diameter and one vacant spot in a p orbital.
Halogen
Halogens combine with the electron-shedding what group.
Halogen combine with the electron-shedding Alkali Metals of Group 1. Table Salt, NaCl, is a prime example of an Alkali-Halogen Compound.
Group in P-Block Elements that have 7 valence electrons according to the PowerPoint?
Halogens
What P-Block Elements Group or Family form compounds with metals (salts)
Halogens
What group in P-Block Elements are reactive nonmetals that tend to gain 1 electron?
Halogens
What is Group 17 in P-Block Elements according to the PowerPoint?
Halogens
What is Group VIIA called
Halogens
Describe the Halogens Group or Family as listed under P-Block Elements as listed in the PowerPoint.
Halogens -Group 17 -Form compounds with metals (salts); a salt is a combination of metal and a halogen -Reactive nonmetals that tend to gain 1 electron -Contains 7 valence electrons
What are the properties of Transition Metals
Have properties that vary from extremely metallic, at the left side, to far less metallic, on the right side
Electronic configuration for Helium
Helium 1s² Helium, He, adds a second electron to this s orbital. Now shell 1 is full and we write 1s²
In relation to how many valence electrons elements have, what element is the exception
Helium as it has only 2 electrons in its outer shell
What is the reactive state of Alkaline Earth Metals?
Highly reactive
Increasing the number of electrons changes the reactivity of the element in predictable ways based on what?
How those electrons fill successive energy levels
Electronic configuration for Hydrogen
Hydrogen 1s¹ Hydrogen, H, has one electron. It must be in the lowest shell's s orbital. We write this as 1s¹
How many valence electrons does Hydrogen (H) have?
Hydrogen (H) has one valence electron because it's in Group IA
If an atoms gains or loses one or more electrons, it is now what?
If an atom gains or loses one or more electrons, it is now an ion and has either a positive charge or a negative charge
Describe halogens
In nature, the reactive halogens tend to bond with metals to form salts, such as sodium chloride (NaCl)
What is the advantage of creating a table in which elements with similar properties were grouped together
In this way, properties of undiscovered elements could be predicted
Ionization Energy Periodic Trend according to the PowerPoint?
Increases from left to right across a period (generally) and know why
Electron Affinity Periodic Trend according to the PowerPoint?
Increases from left to right across a period and know why
Electronegativity Periodic Trend according to the PowerPoint?
Increases from left to right across a period and know why.
What are the F-Block Elements often called according to the PowerPoint?
Inner Transition Metals
How many valence electrons does Iodine (I) have?
Iodine (I) has seven valence electrons because it's in Group VIIA
At atom or group of elements that bears a positive or negative charge
Ion
the radii of the most common ions of the elements.
Ionic Radii
The energy required to remove one electron from the outer shell of an atom
Ionization Energy
To raise an electron from shell 1 to shell 2 requires an energy equal to the difference. In a hydrogen that is (-3.4) - (-13.6) = 13.6 - 3.4= 10.2 eV. To remove an electron complete and make a hydrogen ion required 13.6 eV. This is called the atom's what?
Ionization Energy
Elements are so insistent about having filled valence shells that they'll gain or lose valence electrons to do so. Atoms that gain or lose electrons in this way are called what?
Ions
We can also visualize the electron a as wave, beaming around the nucleus. Quantum mechanics tells us that the electron is always a "standing wave." That is it "goes around" the nucleus a ___ but never a fractional value
It "goes around" the nucleus as a whole number of wavelengths: 1, 2, 3, 4, etc. but never a fractional value. Note: in other words, only certain discrete "orbits" are available to an electron in an atom
Fluorine has what distinguishing quality?
It is the most electronegative atom
The formula of these ionic crystals is given "in lowest terms." Even though a Sodium Chloride Crystal may contain trillions of atoms, we write what?
Its empirical formula Ex. NaCl This shows that the crystal has one sodium ion for each chloride.
What do you need to know in general about the trends in the Periodic Table according to the PowerPoint?
Know the following about each trend -General tend across a period and down a group -How that trend relates to 2 things ----Effective Nuclear Charge Principle energy levels
What series in F-Block Elements have similar reactivity with Group 2 elements?
Lanthanide Series
What series in F-Block elements are silvery metals?
Lanthanide Series
Describe the Lanthanide Series as listed in the PowerPoint.
Lanthanide Series -Silvery Metals -Similar reactivity with Group 2 elements
What are the two F-Block Elements according to the PowerPoint?
Lanthanide Series Actinide Series
What are the F-Block Elements?
Lanthanides Actinides
What is the location of the transition metals?
Large central block of the periodic table
Electronic configuration for Lithium
Lithium 1s²2s¹ Lithium, Li, has to put the third electron in a new shell, shell 2
How many electrons will be gained or lost by Lithium when forming an ion?
Lithium (Li) loses one electron, forming the lithium cation Li+
You can predict how many electrons an atom will gain or lose to become an ion. Group IA (Alkali Metal) elements gain or lose how many electrons?
Lose one electron
You can predict how many electrons an atom will gain or lose to become an ion. Group IIA (Alkaline Earth Metal) elements gain or lose how many electrons?
Lose two electrons
Electronic configuration of Magnesium
Magnesium, MG Ne3s² Magnesium, Similarly we can write this as Ne3s² indicating two s electron orbiting outside a group of electrons just like Neon's. After 2p fills up, the lowest-energy orbital is 3s, in the third shell, followed by 3p
Easy to shape
Malleable
can be beaten into fine sheets
Malleable
Electron Affinity
Measures an atom's "willingness" to become an anion, i.e. to add an extra electron
Who arranged the elements in order of increasing atomic mass
Mendeleev
Who arranged the elements in order of increasing atomic mass?
Mendeleev
Who created a table in which elements with similar properties were grouped together
Mendeleev
Is the following element metal or nonmetal - Bismuth
Metal
Is the following element metal or nonmetal - Chromium
Metal
Is the following element metal or nonmetal - Strontium
Metal
The elements bordering the staircase are called what?
Metalloids
What group would be considered ambivalent when it comes to electrons?
Metalloids
Do metals or nonmetals share electrons among themselves, forming, tightly-packed dense solids.
Metals do share electrons among themselves, forming tightly-packed, dense solids.
For metals, what happens to electrons in bonding?
Metals lose electrons in bonding
Do metals or nonmetals give up electrons freely?
Metals tend to give up electrons freely
Do metals shed or acquire electrons?
Metals tend to shed electrons
Which are more numerous metals or nonmetals?
Metals vastly outnumber nonmetals
The periodic table is broadly divided along a stairstep border into metals and nonmetals, with a few confused "metalloids" straddling the fence. Metals are located on which side?
Metals, on the left, vastly outnumber nonmetals
Who arranged atoms according to increasing atomic number
Moseley
Who arranged atoms according to increasing atomic number?
Moseley
Who arranged atoms according to increasing atomic number
Mosely
Moving left to right along a row of main group elements, the number of outer electrons does what?
Moving left to right along a row of main group elements, the number of outer electrons goes up steadily. Group 1 elements all have one outer electron Group 2 elements have two, etc. until the last group, which all have eight. Note Transition metals have either one or two outer electrons
Moving rightward along a row, electrons are closer to the nucleus, which holds them more tightly, so ionization erngies should what?
Moving rightward along a row, electrons are closer to the nucleus, which holds them more tightly, so ionization energies should rise to a maximum in the last column.
Going along a row from left to right, atoms get smaller, and moving down a column, they get bigger - what is the reason?
Moving to the right, the bigger charge of the nucleus pulls electrons closer in. Going down a column, the outer electrons are in higher shells, hence farther away from the nucleus.
What type of ion is nitrogen most likely to form?
N3- (3 is superscript), also known as nitride or the nitrogen anion. By gaining three electrons, nitrogen, which is in Group VA, assumes a full octet, like neon.
Anions
Negative Ions
Electronic configuration for Neon
Neon, Ne 1s²2s²2p⁶ Neon, Ne, completes shell 2
Electronic configuration for Nitrogen
Nitrogen 1s²2s²2p³ Nitrogen, N, adds an electron to the third p orbital
In its guise as a particle, an electron inhabits a sort of "probability cloud" - NOT a circular orbit. The densest parts of the cloud are where the electron is likeliest to "be" - if it can be said to be anywhere. Are all the clouds round?
No
Groups are often called families because the elements that make up the groups or families have similar chemical properties. Argon (Ar) is part of Group VIIIA. It is a rather unreactive gas. Since families or groups of elements have similar properties, would you expect Krypton (Kr) to be a highly reactive gas?
No. (all of the elements in Group VIIIA are rather unreactive)
Because all Group VIIIA elements are rather unreactive and are gaseous at room temperature, they have been named the noble gas family. An element in Group VIIIA may be generalized by its family name as a(n) ___ gas.
Noble
Elements in the 8th column already have a complete outer shell. These elements are nonreactive and are called what?
Noble Gases
What P-Block Elements Group or Family is colorless?
Noble Gases
What group in P-Block Elements are unreactive?
Noble Gases
What groups already has as many electrons as is necessary?
Noble Gases
What is Group 18 in P-Block Elements according to the PowerPoint?
Noble Gases
What is Group VIIIA called
Noble Gases
Describe the Noble Gases Group or Family as listed under P-Block Elements as listed in the PowerPoint.
Noble Gases -Group 18 -Colorless -Unreactive -Contains 8 valence electrons - except helium which has 2
Group in P-Block Elements that has 8 valence electrons according to the PowerPoint with one exception?
Noble Gases (Contains 8 valence electrons except helium which has 2)
Is the following element metal or nonmetal - Fluorine
Nonmetal
Is the following element metal or nonmetal - Selenium
Nonmetal
Nonmetals are located on what side of the steplike line in the periodic table
Nonmetals are located on the right side of the steplike line in the periodic table.
For nonmetals, what happens to electrons in bonding?
Nonmetals gain electrons in bonding (staircase)
Do metals or nometals generally prefer to gain or share electrons
Nonmetals generally prefer to gain or share electrons
Do nonmetals tend to shed or acquire electrons?
Nonmetals tend to acquire them
Do metals or nonmetals usually have a less cohesive structure.
Nonmetals usually have a less cohesive structure
What is a full shell of eight valence electrons called?
Octet
The p orbitals are aligned on the what?
On the x, y, and z axes
Atomic Radii
One-half the distance between the nuclei of identical atoms that are bonded together
Atomic Radii What is It according to the PowerPoint?
One-half the distance between the nuclei of identical atoms that are bonded together.
Describe nonmetals?
Opposite to that of metals NOT solid and shiny so dull Does NOT conduct electricity and heat Does NOT give up electrons Is NOT malleable or easily shaped Is NOT ductile or easily drawn out into wire
Orbitals are aligned to what within their repsective sublevels?
Orbitals are aligned to axes within their respective sublevels
Electronic configuration for Oxygen
Oxygen 1s²2s²2p⁴
Chlorine (₁₇Cl) is an example of an atom in which the last subshell is not completely filled. Its electron configuration is 1s²2s²2p⁶3s²3p⁵. Note that the 3p subshell has only five electrons and all other subshells are filled. Oxygen is another example of an atom in which the last subshell is unfilled. What is its electron configuration?
Oxygen 1s²2s²2p⁴ (2+2+4=8 electrons)
How many electrons will be gained or lost by Oxygen when forming an ion?
Oxygen (O) gains two electrons to form the oxide anion O2- (2 is superscript)
How many valence electrons does Oxygen (O) have?
Oxygen (O) has six valence electrons because it's in Group VIA
What is the shape of p orbitals?
P orbitals are shaped a bit like dumbbells, with two lobes and a narrow waist.
P sublevels can hold how many electrons each?
P sublevels can hold 6 electrons each
With the exception of 2He, the subshell of greatest energy (last subshell) in each noble gas consists of six electrons occupying a(n) (s,p,d,f) subshell.
P subshell Example: ₈₆Rn 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s² 4f¹⁴5d¹⁰6p⁶
Noble Gases, Halogens, Carbon, Boron, Nitrogen, and Oxygen are part of what block of elements according to the PowerPoint?
P-Block Elements (not clear - not all listed on PowerPoint)
The elements Li, Be, B, C, N, O, F, and Ne are all members of a (group, period)
Period
What is the physical and chemical properties of the elements are periodic functions of their atomic numbers?
Periodic Law
Rows in the periodic table are called
Periods
Electronic configuration of Phosphorus
Phosphorus, P Ne3s²3p³ After 2p fills up, the lowest-energy orbital is 3s, in the third shell, followed by 3p
Cations
Positive Ions
What are the electron configurations of the following elements? Potassium (K)
Potassium (K) 1s²2s²2p⁶3s²3p⁶4s¹
Properties of metals
Properties of metals -High Density -High melting point and boiling point -Good electrical conductivity -Shiny -Malleable (easy to shape) -Ductile (easy to stretch into wries) -Reactive with nonmetals
Properties of nonmetals
Properties of nonmetals -Often liquid or gaseous at room temperature -Brittle when solid -Dull-looking -Poor electrical conductivity -Reactive with metals (except for last group)
Responsible for nuclear charge
Proton
In essence, what is the reasons that atoms bond?
Protons have a positive electrical charge, and electrons have negative charge. One of the fundamental laws of physics is that opposite electrical charges attract, so electrons are attracted to protons and vice versa (That's why atoms always have equal numbers of electrons and protons in the first place; its hard to pull electrons and protons apart)
Electrons obey the bizarre rules of modern physics called what?
Quantum Mechanics
