Topic 2 Atomic Structure. IB Chemistry SL Coral Gables Senior High School Ms. Kiely
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1 Topic 2 Atomic Structure IB Chemistry SL Coral Gables Senior High School Ms. Kiely
2 Bell Ringer (i) Calculate the number of neutrons and electrons in one atom of ⁶⁵Cu. (ii) State one difference in the physical properties of the isotopes ⁶³Cu and ⁶⁵Cu, and explain why their chemical properties are the same. Turn in HW: Exercises I HOPE YOU WROTE THE QUESTIONS! Topic 2 Test is on Friday!
3 ANSWER (i) Calculate the number of neutrons and electrons in one atom of ⁶⁵Cu. Neutrons: 36 and Electrons: 29 (ii) State one difference in the physical properties of the isotopes ⁶³Cu and ⁶⁵Cu, and explain why their chemical properties are the same. Physical: ⁶³Cu has a lower boiling point/melting point/ density/greater rate of diffusion than ⁶⁵Cu DO NOT WRITE different masses Chemical: their chemical properties are identical because they have the same number of electrons and Same electron configuration. ELECTRONS DETERMINE THE CHEMICAL BEHAVIOR OF AN ATOM.
4 -Topic 2 TEST is this FRIDAY (11/30)
5 Extra A and Community Service Hours You can only receive 1 A, but you can receive hours for all three drives: -Donations for Humane Society Animal Drive (A and Community Service Hours) -Donations for Lotus House (A and Community Service Hours)
6 Schrödinger and the Electron Cloud -Based on Heisenberg s uncertainty principle, Erwin Schrödinger in 1926 developed a mathematical equation to figure out where an electron might be located within the electron cloud based on its level of energy. -He knew that an electron s location within the electron cloud could not be known for certain- but a probability of where an electron might be could be calculated! -We call areas of high probability of where an electron might be an atomic orbital.
7 Atomic orbitals describe the three-dimensional areas where there is a high probability that the electron will be located. They are regions around an atom s nucleus in which there is a 90% probability of finding the electron. Shapes of orbitals will depend on the energy of the electron and its motion in that area. When an electron is in an orbital of higher energy, it means it is most likely far from the nucleus. s orbitals are spherical p orbitals are dumbbell-shaped. There are three of them, located on an x, y, and z axis.
8 Why are noble gases typically inert or nonreactive? Meaning, why do the atoms of noble gases not easily bond with other atoms? Noble gases entirely fill their outermost s and p sublevels with electrons, making them have 8 valence electrons. Filled sublevels are more stable than partially filled ones. All atoms want to be stable like the noble gases- a stable atom doesn t spend a lot of energy! Therefore, we say that all atoms* try to achieve noble gas electron configurations; they try to achieve the octet rule by having 8 valence electrons, just like the noble gases. *Hydrogen and Helium are exceptions. They only need 2 valence electrons to be stable. Transition metals are also exceptions. Many want 18 valence electrons to be stable.
9 Valence Electrons We consider electrons to be the most mobile particles of the atom. They are able to be shared with other atoms, gained by atoms, and lost by atoms. Without electrons, we would have no chemical bonds between atoms. The electrons specifically involved in bonding are the outermost electrons of an atom, we call these the valence electrons. Valence electrons are the electrons found on the outermost occupied energy level of an atom.
10 Groups: Columns are referred to as groups. The group number is equivalent to the amount of valence electrons in an atom of that group. Periods: Rows are referred to as periods. The period number is equivalent to the amount of energy levels that electrons occupy at ground state for the atoms of that element.. Ex/Period 3: The electrons of Na, Mg, Al, Si, P, S, Cl and Ar all occupy the first three energy levels.
11
12 Ion: an atom that has a positive or negative charge. Positive and Negative atoms form when they lose or gain valence electrons. When an atom loses an electron it becomes more positively charged since it now has more protons than electrons, and is called a cation. When an atom gains an electron it becomes more negatively charged since it now has more electrons than it has protons, and is called an anion.
13 Metal atoms: Become positive ions by losing all of their valence electrons; electrons located in their highest occupied energy level Positive ions are cations Nonmetal atoms: Become negative ions by gaining enough valence electrons so that their highest occupied energy level is full (has a total of 8 valence electrons) Negative ions are anions
14 Cations: The charge for a cation is written as a number followed by a plus sign. The amount of electrons lost is also included: Anions: The charge for an anion is written as a number followed by a minus sign. The amount of electrons gained is also included: Ex/ if Na loses its 1 valence electron, then the chemical symbol is: Na+ because now Na has 11 protons and 10 electrons. It is more positive by one proton now. Ex/ if Cl gains 1 electron, then the chemical symbol is: Cl because now Cl has 17 protons and 18 electrons. It is more negative by one electron now.
15 Practice What is the charge on the Aluminium (Al) ion?
16 Answer What is the charge on the Aluminium (Al) ion? Answer: Al³+
17 Practice How many electrons does Germanium (Ge) have to give up to achieve a noble-gas configuration?
18 Answer How many electrons does Germanium (Ge) have to give up to achieve a noble-gas configuration? Answer: 4 electrons The chemical symbol would be Ge⁴+
19 Practice How many electrons does nitrogen (N) have to gain in order to achieve a noble-gas configuration?
20 Answer How many electrons does nitrogen (N) have to gain in order to achieve a noble-gas configuration? Answer: 3 electrons The chemical symbol would be N³
21 Practice How does Rubidium (Rb), a metal, obey the octet rule when becoming an ion?
22 Answer How does Rubidium (Rb), a metal, obey the octet rule when becoming an ion? Answer: it loses electrons. Rubidium specifically loses 1 valence electron.
23 Practice
24 Answer Answer: C
25 Electron Despite not being Configuration able to directly detect Diagram the location of an electron directly, scientists like Schrödinger have provided mathematical formulas and theoretical models for us that will help us determine where an electron MOST LIKELY is, as well as where an electron may be traveling to when it absorbs energy and travels away from the nucleus. The formulas can be summarized in something called electron configuration. 1s_ 2s_ 2p _ 3s_ 3p _ 3d _ We will fill in diagonal arrows to help us follow the Aufbau Principle. 4s_ 4p _ 4d _ 4f _ 5s_ 5p _ 5d _ 5f _
26 Electron Configuration Rules 1. Aufbau Principle: lowest energy orbitals are filled first 2. Pauli Exclusion Principle: up to two electrons can occupy an orbital, however they must have opposite spins so as to reduce the repulsion of like charges. (Up arrow means clockwise, down arrow means counter-clockwise.) 3. Hund s Rule: electrons are placed into orbitals of a sublevel one electron at a time, so as to minimize the amount of repulsion in one given orbital. Once all orbitals in a sublevel are filled with one electron, then if more electrons remain a second electron with opposite spin can be added to completely fill the orbital. *SOME transition metals (metals located in groups 3-11) have exceptions to these rules. For IB, you only need to know these exceptions for Cu and Cr.
27 1. State the full electron configuration of vanadium (V) and deduce the number of unpaired electrons. 2. State the full electron configuration of argon (Ar). 3. Identify the excited state in the following electron configurations: a. [Ne]3s²3p³ b. [Ne]3s²3p³4s¹ c. [Ne]3s²3p⁶4s¹ d. [Ne]3s²3p⁶3d¹4s² 4. Which is the correct order of orbital filling according to the Aufbau principle? a. 4s 4p 4d 4f b. 4p 4d 5s 4f c. 4s 3d 4p 5s d. 4d 4f 5s 5p
28 Answers: 1. V: 1s²2s²2p⁶3s²3p⁶3d³4s² There are three unpaired electrons. 2. Ar: 1s²2s²2p⁶3s²3p⁶ 3. b. [Ne]3s²3p³4s¹ 4. c. 4s 3d 4p 5s
29 Electron configurations of ions: -the electron configuration of cations is determined by subtracting electrons that the ion loses out of the outermost occupied orbital(s) of its neutral configuration. -the electron configuration of anions is determined by adding the electrons gained into the next available electron orbital. Example: State the ground-state electron configuration of the Fe²+ ion. When writing the electron configuration of an ion, avoid using the abbreviated/condensed form.
30 Example: State the electron configuration of the Fe²+ ion. Answer: Fe has 26 electrons when neutral. This is the configuration of a neutral atom of Fe:- 1s²2s²2p⁶3s²3p⁶3d⁶4s² The symbol, Fe²+, indicates that this atom of Fe has become a cation by losing two electrons. Since level 4 is the outermost orbital, it contains the valence electrons of this Fe atom. Therefore, we remove the two electrons that reside in 4s. Fe²+: 1s²2s²2p⁶3s²3p⁶3d⁶
31 Practice: Write the full ground-state electron configuration of the following ions: 1) O 2) Ca
32 Answers: 1) O² 1s²2s²2p⁶ 2) Ca²+ 1s²2s²2p⁶3s²3p⁶
33 Rules for writing condensed form electron configurations, a.k.a noble-gas notation In order to write electron configurations in noble-gas notation: Neutral atoms: First, solve for the atom s electron configuration. Then, write the condensed electron configuration using the noble gas in the period BEFORE the atom. Metal ions: First, solve for the neutral electron configuration of the metal atom. Then, remove the valence electrons. THEN, write the condensed electron configuration by using the noble gas that is ONE PERIOD ABOVE that metal s period OR the one that is TWO PERIODS above that metal s period. Both are allowed! Nonmetal ions: First, solve for the neutral electron configuration of the nonmetal atom. Then, add valence electrons until you have a total of 8 valence electrons. THEN, write the condensed electron configuration using the noble gas that is in the SAME period as the nonmetal ion or ONE PERIOD above that metal s period. Both are allowed!
34 PRACTICE Solve for the condensed electron configuration of the following atoms: 1) Sulfur, S 2) Calcium, Ca 3) Rubidium, Rb 4) Carbon, C
35 PRACTICE ANSWERS 1) [Ne]3s²3p⁴ 2) [Ar]4s² 3) [Kr]5s¹ 4) [He]2s²2p²
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