Modern Atom & Periodic Table

Topic: Mass #’s, Atomic #’s, & Isotopes Unit: Modern Atom & Periodic Table Topic: Mass #’s, Atomic #’s, & Isotopes Objectives: Day 1 of 4 To understand the basic components of an atom and how we arrived at this conclusion To understand that an atom is mostly empty space To understand the difference between the mass number and the atomic number To understand how an isotope is different that of a neutral atom

Quickwrite Answer one of the questions below 1-2 sentences: What do you think the modern atom is made of??? What do you think atoms look like??? What do you think happens to atoms during a chemical reaction????

Modern Atom e- e- The modern atom has: Electron Proton Neutron Negatively charged particle that occupies the space around the nucleus (mass = 5.48 x10-5amu) Proton Positively Charged particle in a Nucleus (mass = 1 amu) Neutron A neutral particle in a Nucleus with the same mass as a proton (mass = 1 amu) e- Nucleus size is not scale! P+ N N P+ e-

Actual Size of the Nucleus If an atom was the size of baseball stadium, the nucleus would the size of a pea on the pitcher’s mound, and the electron “cloud” would occupy the size of the stadium

What is the modern atom made of? Answer Bank Carbon-14 Neutrons Same dense Protons negatively Different space space An atom is mostly empty _______ that is made up of a massive electron cloud with a very small ______ nucleus 1 amu is defined in terms of 1/12 the mass of carbon atom dense Proton Neutron Electron Positively Charged particle in a Nucleus (mass = 1 amu) 1 amu = 1.66 x 10-24 gms A neutral particle in a Nucleus with the same mass as a proton _________ charged particle that occupies the space or “cloud” around the nucleus (mass = 5.48 x10-5amu) Negatively

Modern Atom We now know that the modern atom is made up of Protons, Neutrons and Electrons A proton and neutron has the about the same mass of 1 amu (1.66 x 10-24 gms) An electron which occupies the empty space around the nucleus has a mass of 5.48 x10-5amu

Mass Number & Atomic Number Mass Number is basically the mass of the atom Because the electron weighs virtually nothing, we only count the mass of the proton and neutron Remember, a proton and neutron have a mass of 1 amu (atomic mass unit) The atomic number is the number of protons

Mass Number & Atomic Number The Mass Number (#) is the sum of the protons and neutrons So, how many protons does Helium have? How many neutrons Every element has a Mass Number and an Atomic number The Atomic Number is the number of protons The mass number is the sum of protons and neutrons Let’s look at the element Helium The atomic number (#) is the number of protons

What is the difference between the Atomic Number and the Mass Number? The ATOMIC number is the number of ________ in the nucleus of an atom and dtermines the identity of each element The MASS number is the number of protons plus _________ Mass # = (# of protons)+(# of neutrons) Please Draw: protons Answer Bank Carbon-14 Neutrons Same Protons negatively different neutrons

Helium Atom e- e- The HELIUM atom has: 2 protons & 2 neutrons Atomic # = 2 Mass # = 4 What is the charge in the nucleus is Helium has 2 protons? How many electrons are needed to balance a charge of +2 e- P+ N N P+ e-

Isotopes Isotopes are atoms with the same number of protons but different number of neutrons Remember, the number of protons is the atom‘s atomic number (Z) The number of Protons plus Neutrons is the atom’s Mass number (A) To show isotopes we use the symbol: A Z X

One Isotope of HELIUM has: But, if we add two neutrons, Isotopes This Isotope is called Helium-6 One Isotope of HELIUM has: 2 protons & 4 neutrons Atomic # = 2 Mass # = 6 Remember, neutral helium atom has 2 protons and 2 neutrons This is written as: He This is written as: 6 2 But, if we add two neutrons, an isotope forms! He 4 2 e- P+ N N N P+ N e-

Isotopes of Hydrogen H 3 2 1 1 N e- Tritium Deuterium P+ N

Protons Determine the Element Carbon-14 Carbon-12 6 protons 8 neutrons 6 protons 6 neutrons An element doesn’t change just because it has more neutrons, Carbon is still carbon, so long as it has 6 protons Question: What weighs more? 5 atoms of carbon 14 or 5 atoms of carbon-12

U Practice: Determine the amount of Neutrons in the isotope: 238 92 A – Z = # of neutrons 238 - 92 = # of neutrons 146 = # of neutrons

What are Isotopes? Isotopes are atoms with the ______ number of protons but ______number of neutrons same different Answer Bank Carbon-14 Neutrons Same Protons Element different Example: _______, Tritium

C Practice: Determine the amount of Neutrons in the isotope: 14 6 A – Z = # of neutrons 14 - 6 = # of neutrons 8 = # of neutrons

Practice: Complete the table: 207 82 Mass #: ??? Atomic #: ??? Pb 82 Mass #: ??? Atomic #: ??? Protons: ??? Neutrons: ???

Practice: Complete the table: 17 17 20 17 37 Element/Ion Atomic Number Number of Protons Number of Neutrons Number of Electrons Mass Number (protons + neutrons) 17 17 20 17 37

Practice: Na Complete the table: Atomic Number Number of Protons Element Symbol Atomic Number Number of Protons Number of Neutrons Number of Electrons Mass Number Isotope? Yes or No? ?? ?? ?? ?? ?? ?? Element Symbol Atomic Number Mass Number Number of Protons Number of Neutrons Number of Electrons Isotope? Yes or No? Na 23 ?? ?? ?? ?? ?? ?? ??

Cl Summarize: 37 17 What is the modern atom made of? What makes up most of the mass (weight) of an atom? What takes up most of the space of an atom???? How does the size of the nucleus compare to the size of the whole atom? An isotope is…… 37 17 Cl

Topic: Periodic Table & Element Properties Unit: Modern Atom & Periodic Table Topic: Periodic Table & Element Properties Objectives: Day 2 of 4 To understand how the Periodic Table is arranged To understand the reactivity and properties of the different groups

Quickwrite Answer one of the questions below 1-2 sentences: Why do you think the periodic table is organized the way it is???? How do you think the elements vary or change throughout the periodic table?? What do know about metals??? If you can, try listing some physical properties of metals

Periodic Table In every chemistry room, you can expect to see a periodic table The periodic table is listed in order of increasing atomic number It is also arranged in vertical and horizontal columns

Periodic Table Mendeleev, a Russian scientist, arranged the elements by atomic number in 1869 He arranged it this way because of similarities in the chemical properties For example, fluorine and chlorine are gases that react in the same way and are arranged in the same vertical column

Groups Elements with similar chemical Properties that lie in the same vertical column are called groups Groups are often referred to by the number over the column Two or more groups make up a family

Groups Groups are often referred to by the number over the column 17 18 1 2 Groups are often referred to by the number over the column 13 14 15 16 3 4 5 6 7 8 9 10 11 12

What are Groups? Elements with similar chemical ________ that lie in the same vertical column properties Answer Bank Two Properties Right Electricity Separate gases

Alkali Metals Group 1 Alkali metals are elements such as Lithium, Sodium, and Potassium These metals share similar chemical properties with each other They are also very reactive and almost always bonded to another element (Ex. NaCl) In group 1 we have The Alkali Metals

the Alkaline Earth Metals Group 2 Alkaline earth metals include elements such as Beryllium, Magnesium, and Calcium These metals share similar chemical properties In group 2 we have the Alkaline Earth Metals

Halogens In group 17 we have the Halogens Group 17 Halogens include elements such as Fluorine, Chlorine and Bromine Many of these elements are gases or liquids at room temperatures

Noble Gases Group 18 Noble Gases include elements such as Helium, Neon, and Argon As their name implies, these elements are gases at room temperature Noble gases do not react with other elements For example, Helium is always pure helium In group 18 we have the Noble Gases

Transition Metals Transition metals include many of the elements we are familiar with such as Nickel, Iron, Copper, Gold and Silver Most of the elements are Metals In groups 3-12, we have the Transition Metals

What are the different types of groups? Group 1 = Alkali Metals (very reactive) Group 2 = Alkaline Earth Metals Groups 3-12 =Transition Metals Group 17 = ______ Group 18 = Noble Gases (non-reactive, like to be alone) Answer Bank Two Properties Right Electricity Separate halogens Halogens

Physical Properties of Metals Conduct Electricity Malleable (they can be hammered & flattened into thin sheets) Ductile (pulled into wires) Lustrous (shiny)

Physical Properties of Metals For example, copper is a shiny (lustrous) metal that is an excellent conductor of electricity and can be pulled into wires (ductile) Many other metals such as aluminum, Iron, and gold share similar properties with copper

What are some Physical Properties of Metals? Conduct electricity ________ ( they can be hammered & flattened into thin sheets) Ductile ( pulled into wires) Lustrous (shiny) Malleable Answer Bank Two Properties Right Malleable Separate gases

Metals, Semimetals, & Nonmetals The periodic table is also classified into 3 basic different types of substances: -Metals -Semimetals -Nonmetals

Nonmetals Metals Semi Metals

Nonmetals Nonmetals are just like they sound: elements that lack properties of metals (i.e., they do not conduct electricity & they are brittle) They also show much more variation that metals do Examples would include the oxygen (gas), chlorine (gas), bromine (liquid), sulfur (solid), and carbon (solid)

What are Nonmetals? right Elements on the ______ side of the periodic table that do not have properties of metal ( brittle, do not conduct electricity, not shiny) Ex: Sulfur, Carbon Answer Bank Two Properties Right Electricity Separate gases

Semi Metals The elements that divide the Metals and Nonmetals are semimetals These elements are also called Metalloids They have properties of both Metals and Non metals Examples of Silicon (used in computers), and germanium and arsenic

What are semimetals? seperate Elements that ________ metals and nonmetals and have properties of both metals and nonmetals Ex: Silicon and Arsenic Answer Bank Two Properties Right Electricity Separate gases

Metals Conduct Electricity Malleable ( they can be hammered & flattened into thin sheets) Ductile ( pulled into wires) Lustrous (shiny)

Natural States of the Elements As we have seen, matter exists in elements, compounds and mixtures Some elements such as sodium are very reactive and readily bond with other elements Other elements like gold, platinum and Helium are non-reactive and do not like to bond with other elements

Noble Gases Ar If you remember, noble gases, such as helium, neon and argon are non-reactive and exist in nature as single molecules (monoatomic) or atoms Ar He He

Diatomic Molecules Some elements are found in their natural state as diatomic molecules Air is a mixture of N2 and O2 These molecules exist in nature as diatomic molecules A diatomic molecule is a molecule made up of 2 atoms O F

Other Diatomic Molecules at Room Temperature = Gases: H2 ,O2 , N2 , F2 & Cl2 = Liquids: Br2 = Solid: I2

What are the 7 naturally occurring diatomic molecules? Cl A molecule that exists in it’s natural state, made up of _____ atoms: Examples are: H2 ,O2 , N2 , F2 , Cl2 , I2 and Br2 Answer Bank Two Properties Right Electricity Separate gases two O F

Summary What group of elements are very reactive? What do we call them? What group of elements are inert, or non-reactive and like to be alone? What do we call them? Most elements are from what group? Explain on the periodic table where the following can be found: nonmetals, semimetals, metals

Topic: Ions & Ionic Compounds Unit: Modern Atom & Periodic Table Topic: Ions & Ionic Compounds Objectives: Day 3 of 4 To learn how an ion forms To understand the difference between a cation and anion To learn how to balance charges in ionic compounds

Quickwrite Answer one of the questions below 1-2 sentences: So far we have seen that an atom has an equal of amount of protons and electrons; but, what do you think happens when atoms lose or gain electrons??? What do you think atoms or elements do when they bond together???? What do know about metals??? If you can, try listing some physical properties of metals

Ions So far we have seen that an atom has an equal of amount of protons and electrons This results in an exact balance of positive and negative charges A balance of charges means the atom has a neutral charge (or charge of zero) A neutral sodium atom has 11 (+) protons balanced by 11 (-) electrons (+11)+(-11) = 0 neutral

Sodium (Na) Atom e- e- e- e- e- e- e e- e- e- e- P+ N P+ N P+ N P+ P+ A neutral sodium has 11 (+) positive protons balanced by 11 negative electron (-) going around the nucleus e- e- e- e- e- P+ N P+ N P+ N P+ P+ P+ N P+ P+ N N N P+ P+ P+ P+ N e- e e- e- e- e-

Ions Now, what would happen if we added or removed an electron? An Ion would form! An Ion is an atom(s) that has lost or gained one or more electrons giving it an overall charge Ions form when electrons are either added or removed

1+ Sodium (Na) Atom e- e- e- e- e- e- e- e- e- e- e- What would happen if we removed 1 negative electron? e- e- e- A Sodium Ion would form! e- What do you think the charge of this Ion is? e- e- P+ N P+ N P+ N P+ P+ P+ N P+ P+ N N N P+ P+ P+ P+ N e- Because it has one more proton than electrons, it has a charge of 1+ e- e- e- e-

What is an Ion? An atom(s) that has lost or _____ one or more electrons giving it an overall charge Example: Na+1 & Cl1- Answer Bank Addition Metal Negatively removal Positively melting

Cation A cation is a positively (+) charged ion that is formed by the removal of an electron For example, sodium forms a positive +1 ion The Sodium cation lost only one electron, giving it a charge of +1 But, what if an atom lost 2 electrons? For example, magnesium typically loses 2 electrons to form a +2 cation

2+ Magnesium (Mg) Atom e- e- e- A cation with a 2+ charge would form! What would happen if we removed 2 negative electron? e- e- A cation with a 2+ charge would form! e- e- e- P+ N P+ N P+ N P+ P+ P+ N P+ P+ N N N P+ P+ P+ P+ N e- e- e- e- e- e-

Cation 1+ A cation is named using the parent atom For example, Na+ is called the sodium Ion, Mg2+ is called the Magnesium Ion, and is Al3+ called the Aluminum Ion Ex: Na Na+ + 1e- Mg Mg2+ + 2e- 1+

Anion When electrons are gained by a neutral atom, an ion with a negative charge is formed An anion is a negatively charged ion that is formed by the addition or gaining of an electron An atom that gains one extra electron forms an anion with a 1- charge

1- Chlorine (Cl) Atom e- e- e- e- e- e- e- e- e- e- e- What would happen if we added 1 negative electron? e- e- e- e- e- A chlorine ion would form! e- e- e- What do you think the charge of this Ion is? e- e- P+ N P+ N P+ N e- e- P+ P+ P+ N P+ P+ N N e- N P+ P+ P+ e- P+ N e- Because the chlorine atom has (17+) positive protons and (18-) negative electrons, it now has a 1- charge e- e- e- e- e- e- e- e-

Anion Unlike a cation, which is named for the parent atom, an anion is named by taking the root name of the atom changing the ending For example, when a chlorine atom becomes an anion, it is called the chloride ion Cl- Notice: The word chloride is combination of the root word (Chlor-) combined with suffix ending in (–ide) Another example would include the flourine anion: F + 1e- F- (Flouride ion) 1-

Cation and Anions It is important to remember that ions are always formed by removing or adding electrons Ions are never formed by changing the number of protons in the atoms nucleus!

What is the difference between a Cation & Anion? Answer Bank Addition Metal Negatively removal Melting cation A _____ is a positively charged ion formed by the ______ of an electron Ex: Na Na+ + 1e- Name: Sodium ion A anion is a________ charged ion formed by the ________or gaining of an electron Ex: Cl + 1e- Cl- Name: Chloride ion

Ions & the Periodic Table The periodic table is a useful tool when determining what type of ion is formed by a given atom Group 1 metals (Li, Na, K) form 1+ cations Group 2 metals (Be, Mg, Ca) for 2+ cations Note: Metals like to lose electrons and as a result, always form positive ions Nonmetals, on the other hand, form negative ions by gaining electrons Group 17 nonmetals (F, Cl, Br) form 1- anions Group 16 nonmetals (O, S, Se) form 2- anions

Group determines Charge 1+ Cations 2+ Cations 3+ Cations 2- Anions 1- Anions

Practice: #1-4 and write the charge and the name for the following ions…. Cl O Ca = Na+1 = Cl-1 = O-2 = Ca+2

What determines the charge of an ion? The group determines the charge of each ion Group 1 = 1+ Group 2 = 2+ Group 16 = 2- Group 17 = 1- Groups 3-12 = multiple charges

Ionic Compounds Many compounds, such as salt (NaCl-sodium Chloride), are ionic compounds (substance made of 2 or more atoms) In order to melt salt, it needs to be heated to about 800ºCelsius to melt As a solid, salt will not conduct electricity But, when salt is dissolved in water, it will conduct electricity Salt forms when sodium (Na) and chlorine (Cl) ions attract each other

Ionic Compounds Salt forms when sodium and chlorine ions come together Na+ Salt forms when sodium and chlorine ions come together Their positive and negative charges attract each other forming an ionic compound Cl-

Ionic Compounds Many substances are made of ionic compounds Whenever a compound forms between a metal and a nonmetal, it is most likely an ionic compound Ionic compound have high melting points and they conduct electricity when dissolved in water Ionic compounds must have a charge of zero Their must be positive ions (cations) & negative ions (anions) present

An Ionic Compound forms between a metal and nonmetal

What are ionic compounds? A compound that results when a _______reacts with a nonmetal to form a cation and an anion Ionic compounds have high _____points and conduct electricity when dissolved in water Answer Bank Addition Metal Negatively removal Positively melting

Balancing Ionic Compounds Let us look at salt again: NaCl Each sodium ion has a charge of 1+ charge, and each chloride ion has a 1- charge, so they must occur in equal number to give a net charge of zero Cl- Na+ (Charge 1+) + (Charge 1-) = Net Charge: 0

Balancing Ionic Compounds Chlorine (Cl) is A 1- Anion Sodium (Na) is a 1+ Cation Cl- Na+ (Charge 1+) + (Charge 1-) = Net Charge: 0

Ions & the Periodic Table 1+ Cations 2+ Cations 3+ Cations 2- Anions 1- Anions

Balancing Ionic Compounds Let us look at one more ionic compound: MgCl2 The Magnesium ion has a charge of 2+ charge, and each chloride ion has a 1- charge How many chloride ions will I need to Magnesium yield a net charge of zero? Cl- Mg 2+ Cl- (Charge 2+) + 2(Charge 1-) = Net Charge: 0 MgCl2

Balancing Ionic Compounds 2+ Cations 1- Anions Cl- Mg 2+ Cl- (Charge 2+) + 2(Charge 1-) = Net Charge: 0 MgCl2

Balancing Ionic Compounds 2+ Cations 1- Anions F- Ca2+ F- (Charge 2+) + 2(Charge 1-) = Net Charge: 0 CaF2

Balancing Ionic Compounds Potassium (K) is a 1+ Cation Oxygen (O) is A 2- Anions K+ O2- K+ 2(Charge +1) + (Charge 1-) = Net Charge: 0 K2O

Practice: #1-5 and write the formula for the following ionic compounds: ?(+2) + ?(-1) = 0 Ca2+ & Cl-1 Na+ & S2- Al3+ & O2- Mg2+ & O2- K+ & Cl-  CaCl2 1 2 ?(+1) + ?(-2) = 0  Na2S 2 1 ?(+3) + ?(-2) = 0  Al2O3 2 3 ?(+2) + ?(-2) = 0  MgO 1 1  KCl ?(+1) + ?(-1) = 0 1 1

Summarize: Ions form by the ______ or addition of an ________ Group 1 metals have a charge of _____ Group ___ metals have a charge of +2 Group 16 metals have a charge of _____. Group _____metals have a charge of -1 Write the ionic compound that forms between Ca 2+ and F-

Topic: Periodic Table Trends Unit: Energy and Periodic Trends Topic: Periodic Table Trends Objectives: Day 4 of 4 To learn about ionization energy and how it relates to the periodic table To learn about electronegativity and how it relates to the periodic table To learn about atomic radius and how it relates to the periodic table

Quickwrite Answer one of the questions below 1-2 sentences: If you recall, which group of the periodic table readily gives up electrons to form cations?? If you recall, which group of the periodic table readily gains electrons to form anions?? For atoms that LOSE electrons, how do you think this affects their size??? For atoms that GAIN electrons, how do you think this affects their size???

Atomic Properties Science is based on observations and discoveries For example, certain observations about substances will help us better understand our world We know that wood burns, steel rusts, plants grow, and sugar tastes sweet A better understanding of how atoms and molecules behave is crucial to helping us explore our natural world The periodic table is an important tool in helping us understand why atoms have predictable characteristic properties The objective is to understand the general trends or patterns in atomic properties in the periodic table

Metals, Semimetals, & Nonmetals If you recall, the periodic table is divided into 3 basic different types of elements: -Metals -Semimetals -Nonmetals

Nonmetals Metals Semi Metals

Atomic Properties & the Periodic Table 1+ Cations 2+ Cations 3+ Cations 2- Anions 1- Anions If you recall, group 1 metals like to lose an electron and group 2 metals like to lose an two electrons, becoming positively charged Non metals on the other hand, like to gain electrons and become negatively charged

Atomic Properties & the Periodic Table Lithium is the least likely to lose an electron Cesium loses an electron most easily But what elements in group 1 are the most likely to lose an electron? Not all metals in group 1 behave exactly the same way For example, some metals can lose one or more electrons much more easily than others Cesium at the bottom of group 1, gives up an electron much more easily than lithium at the top of group 1

Atomic Properties & the Periodic Table In fact, as we go down the periodic table, the metals in group 1 become more likely to lose an electron Cs > Rb > K > Na > Li Cesium loses an electron most easily Lithium is the least likely to lose an electron

Atomic Radius (Size) What do you notice about the relative sizes of Group 1 Atomic Radius (Size) Period 4 What do you notice about the relative sizes of the atoms as we move up group 1? That’s right the atomic radius gets smaller! What do you notice about the relative sizes of period 4 atoms as we move across the periodic table left to right? That’s right the atomic radius gets smaller!

Atomic Radius (Size) Atomic Size Decreases Atomic Size Decreases

Atomic Size Cs Na What makes the atomic size get bigger? Li What makes the atomic size get bigger? Their nucleus and electron cloud size becomes larger Na K Atomic Size Decreases Rb Atomic Size Decreases Cs Na Mg Al Si P S Cl Ar

How does atomic Size Change across the Periodic table? Atomic size ________ as we go up the periodic table and decreases as we go left to right Their nucleus and electron cloud gets ________ Draw: decreases Answer Bank Weakly larger Attract remove Decreases low larger Decreases

Ionization Energies The ionization energy is the energy required to remove an electron from an individual atom Think of it as how easily an atom loses an electron Metals have low ionization energies, and nonmetals tend to have higher ionization energies

1+ Sodium (Na) Atom e- e- e- e- e- e- e- e- e- e- e- How much energy is required to remove an electron from a sodium atom? e- e- e- Recall that sodium likes to lose an electron to form a +1 ion e- e- e- e- P+ N P+ N P+ N P+ P+ P+ N P+ P+ N N In general, metals such as sodium have low ionization energies (they require very little energy to lose an electron) N P+ P+ P+ P+ N e- e- e- When atoms such as sodium lose electrons, their atomic size or radius decreases e- e-

Ionization Energy What do you notice about the relative sizes of Energy Increases What do you notice about the relative sizes of the atoms as we move up from cesium to Lithium? That’s right the atomic size gets smaller! Ionization Energy Increases Notice the Ionization Energy trend

What is Ionization Energy? The energy required to ______ an electron from an individual atom Metals (group 1 & 2) have _____ ionization energies and nonmetals (group 17 halogens & group 18 noble gases) have high ionization energies Draw: remove Answer Bank Weakly larger Attract remove Decreases low low Increases

Electronegativity If Ionization energy is how easily an atom loses an electron, then think of electronegativity as the exact opposite Electronegativity is the ability of an atom to attract electrons Think of it as the liking or attraction an atom has for an electron Nonmetals such as Flourine, chlorine and oxygen have high electronegativities In other words, Flourine, Chlorine and Oxygen love to steal electrons form other atoms

Electronegativity What do you notice about the relative sizes of Increases What do you notice about the relative sizes of the atoms as we move up from cesium to Lithium? That’s right the atomic size gets smaller! Notice the Electronegativity trend Electronegativity increases

What is Electronegativity? Ability of an atom to _______electrons Nonmetals such as Fluorine, Chlorine and Oxygen have high electronegativities along with noble gases such as Helium and argon Draw: attract Answer Bank Weakly larger Attract remove Decreases low Increases

Electronegativity vs. Ionization Energy What determines Ionization energy and Electronegativity? The answer is atomic radius! Larger atoms lose Electrons easier because the outer electrons are farther from the nucleus, & are therefore more weakly held P+ N P+ N P+ e- N P+ P+ P+ N P+ P+ N N N P+ P+ P+ P+ N

Electronegativity vs. Ionization Energy What determines Ionization energy and Electronegativity? The answer is atomic size! Smaller atoms like fluorine hold their outer electrons are closer to the Nucleus and therefore do not Lose their electrons as easy This also enables them to steal Electrons from other atoms (High electronegativity) e- P+ N P+ N P+ N e- P+ P+ P+ N P+ P+ N N N P+ P+ P+ P+ N

The more Electronegative Atom, Fluorine in this case, steals the weakly held outer electrons from Cesium e- P+ N P+ N P+ e- N P+ N P+ N P+ P+ P+ P+ N N e- P+ P+ N P+ P+ P+ N N P+ P+ N N P+ P+ N P+ P+ N N P+ P+ P+ P+ N Fluorine Cesium

e- e- P+ N P+ N P+ N P+ N P+ N P+ P+ P+ P+ N N P+ P+ N P+ P+ P+ N N P+ Because Fluorine gains an electron, it’s atomic radius becomes larger, and because cesium loses an electron, it’s atomic radius becomes smaller e- P+ N P+ N P+ N P+ N P+ N P+ P+ P+ P+ N N e- P+ P+ N P+ P+ P+ N e- N P+ P+ N N P+ P+ N P+ P+ N N P+ P+ P+ P+ N Fluorine Cesium

How does atomic size effect ionization energy and electronegativity? Larger atoms (cesium) with low ionization energies ______ hold their outer electrons and easily lose them Smaller atoms (fluorine) with high electronegativities strongly hold their electrons closer to the nucleus and steal electrons from other atoms Answer Bank Weakly larger Attract remove Decreases low weakly

Summarize: List 3 atoms with a large atomic radius: Explain where atoms with low ionization energies can be found: List 3 examples: Explain where the most electronegative atoms can be found: List 3 examples: Explain where the largest atomic size can be found on the periodic table: