Homework quiz lessons 17-24
Sodium cyanide, NaCN, contains a cyanide ion. What is the charge on the cyanide ion? Lesson 22
-1
Calcium phosphate, Ca(PO₄)₂, contains phosphate ions. What is the charge on a phosphate ion?
-3
What is the total number of subshells for elements in Period 5 of the periodic table? Lesson 24
15
Draw a shell model for boron, B. Identify the core and valence electrons. Lesson 18
2 core electrons (on red circle), 3 valence electrons (on blue circle)
What is the outermost subshell for bromine, Br? Lesson 24
4f subshell
What evidence do you have from flame tests that copper is responsible for producing a flame with a blue-green color? Lesson 17
All the flames that were produced with a blue-green color had copper (Cu) in the compound that was being tested.
Which noble gas is closest to sulfur, S, on the periodic table? What must happen to a sulfur atom for it to have an electron arrangement similar to that of a noble gas? Lesson 19
Argon, Ar Sulfur would have to gain two electrons
What charge would an arsenic, As, ion have? Lesson 19
As³⁻, negative 3 charge
You should be able to figure out the identity of an atom from its electron configuration alone. Describe at least two ways you could do this. Lesson 24
Atomic number and total number of electrons
Explain the difference between an anion and a cation. Lesson 19
Cations have a positive charge, anions have a negative charge
List four ions that have the same number of electrons as argon, Ar. Lesson 19
Cl⁻,S²⁻, Ca²⁺,K⁺
What are ionic compounds, and how do they form? Review summary
Compounds involving ions of elements; formed through chemical reactions
Cobalt violet is a paint pigment discovered in 1859. If the cation for this compound is Co²⁺ and the anion is PO₄³⁻, what is the chemical formula? Lesson 23
Co₃(PO₄)₂
List four ions that have the same number of electrons as neon, Ne. Lesson 19
F⁻, Mg²⁺, Na⁺, O²⁻
What periodic patterns do you notice for the charges of the ions ? Lesson 19
In group 1A they lose an electron making them have a +1 charge, group 2A is a +2 charge, group 3A is a +3 charge, group 4A is a +4 charge, group 5A is a -3 charge, group 6A is a -2 charge, and group 7A is a -1 charge
What does the Roman numeral in a chemical name indicate? Lesson 23
Indicates the charge on the transition metal cation
Explain the importance of valence electrons. Review summary
It determines the amount of atoms that can be used in a chemical reaction
When chlorine gains an electron to become a chloride ion with a -1 charge, it ends up with the electron arrangement of argon. Why doesn't it become an argon atom? Lesson 19
It does not become argon because it does not have the same number of protons.
Explain what is meant by noble gas envy. Lesson 19
It is when highly reactive elements are trying to become a noble gas.
Would it matter whether you did a flame test with sodium chloride, NaCl, in solid form or sodium chloride in an aqueous solution? Explain. Lesson 17
It would not affect the color of the flame because the compound is still the same just in different forms.
Give examples of six ionic compounds with a metal-to-nonmetal ratio of 1:1. Specify the total number of valence electrons for each compound. Name each compound. Lesson 21
LiF: lithium fluoride: 8 valence electrons KBr: potassium bromide: 8 valence electrons NaF: sodium fluoride: 8 valence electrons KF: potassium fluoride: 8 valence electrons NaCl: sodium chloride: 8 valence electrons LiBr: Lithium bromide: 8 valence electrons
Give examples of three ionic compounds with a metal-to-nonmetal ratio of 1:2. Specify the total number of valence electrons for each compound. Name each compound. Lesson 21
MgCl₂: magnesium chloride:16 valence electrons CaBr₂: calcium bromide: 16 valence electrons BeF₂: beryllium fluoride: 16 valence electrons
Give examples of three ionic compounds with a metal-to-nonmetal ratio of 2:1. Specify the total number of valence electrons for each compound. Name each compound. Lesson 21
Na₂O: sodium oxide: 8 valence electrons K₂S: potassium sulfide: 8 valence electrons Li₂O: lithium oxide: 8 valence electrons
Which noble gas is closest to magnesium, Mg, on the periodic table? What must happen to a magnesium atom for it to have an electron arrangement similar to that of a noble gas? Lesson 19
Neon, Ne Magnesium would have to lose two electrons
Does nitrate produce a colored flame? explain your thinking. Lesson 17
No, nitrate does not produce a colored flame because neither of the elements present in the compound are metals and therefore they do not react with the heat from the Bunsen burner.
Predict the color of the flame for the compound sodium hydroxide, NaOH. Explain your reasoning. Lesson 17
The color of the flame will be yellow-orange because Sodium (Na) is present in all the compounds that have a yellow-orange flame.
How did the flame tests provide evidence that specific atoms are present in compounds? Lesson 17
The flame test provided evidence that specific atoms are present in compounds by the color of the flame.
Explain what is responsible for the colors during the flame test. Lesson 17
The metal atoms are what is responsible for the colors during the flame test.
How does the rule of zero charge help you predict the formula of an ionic compound? Lesson 20
The negative charge plus the positive charge has to equal zero. This can help because it can determine how many atoms of a specific element you will need so there is a zero charge.
How is the arrangement of electrons within atoms connected to the periodic table? Review summary
The number of valence electrons relates to what group the element is in and the amount of electron shells relates to what period the element is in
Explain how to use the periodic table to determine the correct formulas for ionic compounds. Lesson 21
The periodic table can provide the name and symbol of the element and based on its location, how many electrons it will lose or gain.
Explain why the following compounds do not form.Lesson 20 a) NaCl₂ b) CaCl c) AlO
The valence electrons do not add up to a zero charge
What do beryllium, Be, magnesium, Mg, and calcium, Ca, all have in common? Lesson 18
They all have 2 valence electrons
Explain why the chemical properties of argon, krypton, and xenon are similar, even though there are 18 elements between argon and krypton and 32 elements between krypton and xenon. Lesson 24
They are in the same group so they have similar properties. They are also noble gases.
Explain why the elements on the right side of the periodic table gain electrons instead of using them. Lesson 19
They need to gain electrons to become the noble gases that are closest to them.
What is the symbol of an ion with 22 protons, 24 neutrons, and 18 electrons? Lesson 19
Ti⁴⁺
How can you use valence electrons to predict which ionic compounds will form? Lesson 20
You can determine how many electrons an atom needs to give away and how many electrons an atom needs to receive and if it is the same amount they can form a compound. It can also show you how many atoms you may need of a specific element to get to zero charge. Ex: Li⁺ and F⁻ can form Lithium fluoride
How can you determine the arrangement of an element's electrons from its position on the periodic table? Lesson 18
You can determine the arrangement by looking at what period they are in which determines the amount of electron shells they have and what group they are in which determines how many valence electrons they have.
If you know what group an element is in, what can you predict about its electron arrangement? Lesson 18
You can predict how many valence electrons are in the valence shell.
Explain how you determine the charge on a transition metal cation from the chemical formula. Lesson 23
You can use the rule of zero charge to determine the charge on a transition metal cation from the formula.
For each of these compounds show that the charges on the ions add up to zero. a) KBr b) CaO c) Li₂O d) CaCl₂ e) AlCl₃ Lesson 20
a) (+1)+(-1)=0 b)(+2)+(-2)=0 c) 2(+1)+(-2)=0 d)(+2)+2(-1)=0 e)(+3)+3(-1)=0
Write the electron configuration for each of these atoms. Then write it using the noble gas shorthand method. Lesson 24 a) oxygen b) chlorine c) iron d) calcium e) magnesium f) silver g) silicon h) mercury
a) (He)2s²2p⁴ b) (Ne) 3s²3p⁵ c) (Ar) 3d⁶4s² d) (Ar)4s² e) (Ne)3s² f) (Kr) 4d¹⁰5s¹ g) (Ne) 3s²3p² h) (Xe) 4f¹⁴5d¹⁰6s²
Lithium nitride has the formula Li₃N a) what is the charge of the lithium ion? b) what is the charge of the nitrogen ion? c) show that the charges of the ions add up to zero d) what is the total number of valence electrons in all the atoms in Li₃N? Lesson 20
a) +1 b) -3 c) 3(1⁺) + 3⁻=0 d) Each lithium has 2 valence electrons and nitride has 8.
Determine the charge on the transition metal cation in each of the compounds listed. Then name each compound. Lesson 23 a) HgS b) CuCO₃ c) NiCl₂ d) Co(NO₃)₃ e) Cu(OH)₂ f) FeSO₄
a) +2 mercury sulfide b)+2 copper (II) carbonate c) +2 nickel chloride d)+3 cobalt (III) nitrate e) +2 copper (II) hydroxide f)+2 iron (II) sulfate
Aluminum arsenide has the formula AlAs a) what is the charge of the aluminum ion? b) what is the charge of the arsenic ion? c) show that the charges of the ions add up to zero d) what is the total number of valence electrons in all the atoms in AlAs? Lesson 20
a) +3 b) -3 c) (+3) + (-3) = 0 d) Each aluminum atom has 8 valence electrons and each arsenic atom has 8 valence electrons
Consider the element with the atomic number 13. Lesson 24 a) what is the electron configuration for the element with atomic number 13? b) how many valence electrons does element 13 have? how do you know? c) how many core electrons does element 13 have? How did you figure that out?
a) 3 electron shells 2, 8, 3 b) 3 valence electrons c) 10 core electrons; subtract the number of valence electrons from the total number of electrons
What are the total numbers of valence electrons in all the atoms in each of these compounds? a) KBr b) CaO c) Li₂O d) CaCl₂ e) AlCl₃ Lesson 20
a) 8 b) 8 c) 8 d) 16 e) 24
Predict the formulas for ionic compounds that are formed when these metal and nonmetal elements are combined. Name each compound. Lesson 21 a) Al and Br b) Al and S c) Al and As d) Na and S e) Ca and S f) Ga and S
a) AlBr₃: aluminum bromide b) Al₂S₃: aluminum sulfide c)AlAs: aluminum arsenide d) Na₂S: sodium sulfide e) CaS: calcium sulfide f)Ga₂S₃: gallium sulfide
Write the cation and anion in each compound, then determine the correct chemical formula. Lesson 23 a) copper (II) sulfide b) nickel (II) nitrate c) iron (II) carbonate d) cobalt (II) sulfate e) iron (III) carbonate f) chromium (VI) oxide
a) Cu²⁺,S²⁻ CuS b)Ni²⁺,NO₃⁻ Ni(NO₃)₂ c) Fe²⁺, CO₃²⁻ FeCO₃ d) Co²⁺, SO₄²⁻ CoSO₄ e) Fe³⁺, CO₃²⁻ Fe₂(CO₃)₃ f) Cr³⁺, O²⁻ Cr₂O₃
Write the chemical formula for each compound listed here. Lesson 22 a) lithium sulfate b) potassium hydroxide c) magnesium nitrate d) ammonium sulfate
a) Li₂SO₄ b)KOH c) MgNO₃ d) NH₄SO₄
For each compound, write the cation and anion with the appropriate charge. Then write the chemical formula for each compound. Lesson 21 EXAMPLE: sodium fluoride, Na⁺F⁻, NaF a) magnesium oxide b) rubidium bromide c) strontium iodide d) beryllium fluoride e) aluminum chloride f) lead sulfide
a) Mg²⁺, O²⁻ MgO b) Rb⁺, Br⁻, RbBr c)Sr²⁺, I⁻, SrI₂ d) Be²⁺,F⁻, BeF₂ e)Al³⁺,Cl⁻, AlCl₃ f) Pb⁴⁺,S⁻, PbS₄
Write the name for each ionic compound listed here. Lesson 22 a) NH₄Cl b) K₂SO₄ c) Al(OH)₃ d)MgCO₃
a) ammonium chloride b)potassium sulfate c)aluminum hydroxide d)magnesium carbonate
For each compound listed, identify the anion and cation and the charge on each. Review summary a) magnesium chloride MgCl₂ b) calcium nitrate, Ca(NO₂)₂
a) cation : Mg²⁺ anion: Cl⁻ b)cation: Ca²⁺ anion: NO₂⁻
Which elements are described by these electron configurations? Lesson 24 a) 1s²2s²2p⁶3s²3p⁶4s²3d⁴ b) 1s²2s²2p⁶3s²3p² c) 1s²2s²2p³ d) 1s²2s²2p⁶2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s¹ e) 1s²2s²2p⁶2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d¹⁰6p² f) (Kr)5s²4d⁹
a) chromium b) silicon c) nitrogen d) promethium e) radium f) sodium
Which of these ions have the same number of electrons as S²⁻? Choose all that apply. Lesson 19 a) Cl⁻ b)Ca²⁺ c)Na⁺ d) O²⁻ e) P³⁻
a, b, and e
Which chemical formulas are consistent with the guidelines for creating ionic compounds? Explain your thinking. Lesson 21 a) LiCl b) LiCl₂ c) MgCl d) MgCl₂ e) AlCl₃
a, d, and e because the metals lose the same amount of electrons the chloride gains.
Which of these ions have the correct charge? choose all that apply. Lesson 19 a) Na²⁺ b)Li⁺ c)Al⁴⁺ d) Ca²⁺ e) Ga³⁺
b and d
Which chemical formula does not represent a possible compound with sulfate,SO₄²⁻? Lesson 22 a) Na₂SO₄ b) KSO₄ c) Al₂(SO₄)₃ d) CaSO₄
b because there is only 1 positive charge on the potassium but 2 on sulfate.
What are electron subshells? Lesson 24
electron shells further divided
How is an arrangement of electrons in an atom related to the location of the atom on the periodic table? Lesson 24
elements in the same group have the same amount of valence electrons and elements in the period have the same number of electron shells
Name an element with electrons in the f subshell. Lesson 24
gadolinium, Gd
What flame color would be produced for Ba(OH)₂? Lesson 17
green because Barium, Ba, is present.
What flame color would be produced for BaO? Lesson 17
green because Barium, Ba, is present.
What is an electron configuration? Lesson 24
how the electrons are arranged in the electron shells
What is a polyatomic ion? Lesson 22
ionic compounds that contain ions that consist of 2 or more elements
Explain how to use the periodic table to determine the charges on ions. Lesson 21
left of the periodic table loses electrons, right of the periodic table gains electrons, and the last column (noble gases) keep their electrons
How many subshells are in each shell: n=1, n=2, n=3, n=4? Lesson 24
n=1 maximum of 2 electrons n=2 maximum of 8 electrons n=3 maximum of 16 electrons n=4 maximum of 32 electrons
What flame color would be produced for KOH? Lesson 17
pink-lilac because Potassium, K, is present.
What flame color would be produced for K₂Co₃? Lesson 17
pink-lilac because Potassium, K, is present.
How many protons, neutrons, and electrons does Li⁺ have? Lesson 19
protons- 3 neutrons- 3 electrons- 2
Give two similarities and two differences between Cl and Cl⁻. Lesson 19
similarities: same atom, same atomic number differences: different charge, different number of electrons
How can you tell from a chemical formula if there is a polyatomic ion in a compound? Lesson 22
two or more capital letters
What flame color would be produced for Na₂Co₃? Lesson 17
yellow-orange because sodium, Na, is present.
