Presentation on theme: "Periodic Table/Electron Configuration/Periodic trend Quiz"— Presentation transcript:
1Periodic Table/Electron Configuration/Periodic trend Quiz What’s the electron configuration of neon?What atomic model is the electron configuration based on?What’s the name of the group that neon is in?List the elements that have both metal and nonmetal characteristics. What do you call these elements?Between S and Cs, which element has bigger radius?
2Why learn electron configuration? Let’s think about what we learned in matter…What is physical property?What is chemical property?Property is determined by valence e-How reactive is element?How do we figure out how many valence electrons are in element?ELECTRON CONFIGURATION!!
4Valence electronDef) electrons in the outermost electron shell of an element.There are 3 ways to figure it out!Let’s do quick review on electron configuration!Carbon’s # of e-=E- configuration=Let’s look the Periodic Table
5Octet ruleElements would like to have 8 electrons in their outermost energy level (highest n value). This means that elements try to get a s2p6 configuration in their highest n value energy level.Which group has all the s & p filled with e-?Many transition metals also lose some of their “d” electrons in addition to the electrons needed to satisfy the octet rule
6One way to divide periodic table is by using electron configuration
7Here’s trivia question! Who came up with basics of periodic table? Dmitri Mendeleev!! Pg. 390
8Noble Gases Outermost s and p sublevels are filled Pg.395 Group 18 Also called as inert gas because of how it isn’t very reactive
9Representative elements Outermost s or p sublevel is only partially filledWhich groups are representative elements?
10Group 1A)alkali metalslithium, sodium, potassium, rubidium, cesium, and franciumAlkali metals are so named because they are metals that react with water to make alkaline solutions.Because the alkali metals have a single valence electron, they are very reactive.
11Group2 Alkaline-Earth metals Which element are alkaline-earth metals?What’s the configuration?Slightly less reactive than alkali metalsUsually found in compoundTakes more energy than alkali metals to fulfill octet rule
12Gp17 Halogens Most reactive group of nonmetal elements Why is it so reactive?Because the alkali metals have one valence electron, they are ideally suited to react with the halogensSalt former
13Transition metalsOutermost s sublevel and nearby d sublevels contain electrons.Group B elementsCan use inner shell before using the outer shell to bondCan lose 1-3 valence electrons depending on the element with which it reacts with
14The Inner transition metal Outermost s sublevel and nearby f sublevel generally contain electronsmany are man made
17Metals, Nonmetals, Metalloids There is a zig-zag or staircase line that divides the table.Metals are on the left of the line, in blue.Nonmetals are on the right of the line, in orange.
18Metals, Nonmetals, Metalloids Elements that border the stair case, shown in purple are the metalloids or semi-metals.There is one important exception.Aluminum is more metallic than not.
19MetalsMetals are lustrous (shiny), malleable, ductile, and are good conductors of heat and electricity.They are mostly solids at room temp.
20Nonmetals Nonmetals are the opposite. They are dull, brittle, nonconductors (insulators).Some are solid, but many are gases, and Bromine is a liquid.
21Metalloids Metalloids, aka semi-metals are just that. They have characteristics of both metals and nonmetals.They are shiny but brittle.And they are semiconductors.What is our most important semiconductor?
23Periodic Trends The first and most important is atomic radius. Using your knowledge of mathematics, figure out how you could measure the radius of an atom.Radius is the distance from the center of the nucleus to the “edge” of the electron cloud.What is this statement assuming?Level 3Level 4
24Atomic RadiusSince a cloud’s edge is difficult to define, scientists use define covalent radius, or half the distance between the nuclei of 2 bonded atoms.2.86 Å
25Atomic RadiusThe trend for atomic radius in a vertical column is to go from smaller at the top to larger at the bottom of the family.Based on what you know, how would you explain the growing size of atom?With each step down the family, we add an entirely new energy level to the electron cloud, making the atoms larger with each step.Level 6
26Atomic Radius The trend across a horizontal period is less obvious. What happens to atom as we step from left to right?Each step adds a proton and an electron.What does this mean in terms of charge?Level 5Level2
27Atomic RadiusThe effect is that the more positive nucleus has a greater pull on the electron cloud.The increased attraction pulls the cloud in, making atoms smaller as we move from left to right across a period.
28Effective Nuclear Charge What keeps electrons from simply flying off into space?Effective nuclear charge is the pull that an electron “feels” from the nucleus.The closer an electron is to the nucleus, the more pull it feels.As effective nuclear charge increases, the electron cloud is pulled in tighter.
29Atomic RadiusOn your periodic table sheet, draw arrows like this:
30Let’s practice!!!Which of the following elements has the largest atomic radius?1. carbon (C) 2. silicon (Si) germanium (Ge) 4. tin (Sn)1. nitrogen oxygen fluorine neonThe atomic radius of F, Br, and I are 64, 114, and 138 pm respectively. From this information (and not your book) estimate a reasonable atomic radius of Cl.1. 53pm pm pm pm
31IonsWhen an atom gains an electron, it becomes negatively charged (more electrons than protons ) and is called an anion.In the same way that nonmetal atoms can gain electrons, metal atoms can lose electrons.They become positively charged cations.
32She’s unhappy and negative. IonsHere is a simple way to remember which is the cation and which the anion:This is Ann Ion.This is a cat-ion.She’s unhappy and negative.He’s a “plussy” cat!
33Ionic Radius Cations are always smaller than the original atom. Who can explain why cation is smaller than original atom?The entire outer PEL is removed during ionization.Conversely, anions are always larger than the original atom.Electrons are added to the outer PEL.
34Cation FormationEffective nuclear charge on remaining electrons increases.What element is this? How may Valence e-?Remaining e- are pulled in closer to the nucleus. Ionic size decreases.11p+Valence e- lost in ion formationResult: a smaller sodium cation, Na+
35Anion FormationA chloride ion is produced. It is larger than the original atom.Chlorine atom with 7 valence e-17p+One e- is added to the outer shell.Effective nuclear charge is reduced and the e- cloud expands.
36Let’s practice Which has the larger radius? 1. Na 2. Na+ 1. O 2. O2- Which has the largest radius?1. K K Rb Rb+
37ShieldingAs more PELs are added to atoms, the inner layers of electrons shield the outer electrons from the nucleus.The effective nuclear charge (enc) on those outer electrons is less, and so the outer electrons are less tightly held.
38Ionization EnergyIf an electron is given enough energy (in the form of a photon) to overcome the effective nuclear charge holding the electron in the cloud, it can leave the atom completely.The atom has been “ionized” or charged.The number of protons and electrons is no longer equal.
39Ionization EnergyThe energy required to remove an electron from an atom is ionization energy. (measured in kilojoules, kJ)The larger the atom is, the easier its electrons are to remove.Why?Ionization energy and atomic radius are inversely proportional.
40Ionization Energy (Potential) Draw arrows on your help sheet like this:
41Let’s practice Which element has greater ionization energy? 1. N 2. O From which element is it harder to pull electron away?1. Be 2. BWhich one has greatest ionization energy?1. beryllium (Be) 2. strontium (Sr) calcium (Ca) magnesium (Mg)Which one has strongest shielding effect?
42ElectronegativityElectronegativityis the tendency for atom to attract electron when they are chemically bonded.(also measured in kJ).
43EN depends on… Atomic size Nuclear charge Greater the size of the atom, the lesser the electronegativityNuclear chargeThe greater the nuclear charge, the greater the electronegativity
44ElectronegativityDraw arrows on your help sheet like this:
45Let’s practice! Which has the highest electronegativity? 1. Na Al S ClWhich element attracts electron least?1. F I Br Cl