Which of the following statements best accounts for the 2p peak being twice the height of the 2s peak?

The intensity of the photo-electron signal at a given energy is a measure of the number of electrons in that energy level.

The height of peaks in a photo-electron spectrum does not have any relation to the structure of an atom.

In a photo-electron spectrum, as binding energy increases the relative number of electrons decreases.

Electrons represented by peak 2s have approximately triple the binding energy than those represented by peak 2p.

Which of the following statements is true regarding Nitrogen and Sulfur?

Nitrogen has a smaller atomic radius and a greater electronegativity.

Sulfur has a smaller atomic radius and a greater electronegativity.

Nitrogen has a larger atomic radius and a larger first ionization energy.

Sulfur has a larger atomic radius and a larger first ionization energy.

The diagram above shows the relative atomic sizes of three different elements from the same period. Which of the following statements must be true? (Select all that apply)

The first ionization energy will be greatest in element Z.

The effective nuclear charge will be the greatest in element Z.

The electronegativity value will be greatest in element X.

The electron shielding effect will be greatest in element Z.

The effective nuclear charge will be the greatest in element X.

AP Chemistry Topic 1

Quiz

•

Chemistry

•

10th - 12th Grade

•

Practice Problem

•

Hard

•

NGSS

HS-PS1-1, HS-PS1-7, HS-PS1-2

Standards-aligned

Charles Martinez

FREE Resource

25 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

According to the following reaction, how many grams of ammonia will be formed upon the complete reactions of 15.8 grams of nitrogen gas with excess hydrogen gas?

9.60 grams ammonia

19.2 grams ammonia

38.4 grams ammonia

4.80 grams ammonia

A sample of a hydrate of Na₂CO₃ with a mass of 550 grams was heated until all the water was removed. The sample was then weighed and found to have a mass of 300 grams. What is the formula for the hydrate?

Na₂CO₃⋅ 4H₂O

Na₂CO₃⋅ 10H₂O

Na₂CO₃⋅ 3H₂O

Na₂CO₃⋅ 5H₂O

Al₂O₃(l) → Al(s) + O₂(g)

Approximately how many liters of oxygen gas will be evolved at STP, if 25.68 grams of alumina decomposes?

22.4 L

8.46 L

5.64 L

11.2 L

4.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

The mass spectrum represented above is most consistent with which of the following elements?

Nb

Zr

Y

Mo

5.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

An element consists of 94.93% of an isotope with mass 31.97 u, 0.76% of an isotope with mass 32.97 u, 4.29% of an isotope with mass 33.97 u, and 0.02% of an isotope with mass 35.97 u. Calculate the average atomic mass, and identify the element.

32.06,S

32.07,P

3206,S

3207,P

6.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

The element boron (B) has two naturally occurring isotopes, ¹⁰B and ¹¹B, with an average atomic mass of 10.812 u. Boron is 80.2 % ¹¹B, and the atomic mass of ¹¹B is 11.009 u. Calculate the mass of ¹⁰B.

10.5 u

11.01 u

10.01 u

10.8 u

7.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

The molecule drawn above has the same empirical formula as another compound "X" with a molar mass of 265.1.

Determine the molecular formula of compound "X".

C₂H₃O

C₄H₆O₂

C₁₂H₁₈O₆

C₈H₁₂O₄

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AP Chemistry Topic 1

25 questions

According to the following reaction, how many grams of ammonia will be formed upon the complete reactions of 15.8 grams of nitrogen gas with excess hydrogen gas?

A sample of a hydrate of Na₂CO₃ with a mass of 550 grams was heated until all the water was removed. The sample was then weighed and found to have a mass of 300 grams. What is the formula for the hydrate?

Al₂O₃(l) → Al(s) + O₂(g)

Approximately how many liters of oxygen gas will be evolved at STP, if 25.68 grams of alumina decomposes?

The mass spectrum represented above is most consistent with which of the following elements?

An element consists of 94.93% of an isotope with mass 31.97 u, 0.76% of an isotope with mass 32.97 u, 4.29% of an isotope with mass 33.97 u, and 0.02% of an isotope with mass 35.97 u. Calculate the average atomic mass, and identify the element.

The element boron (B) has two naturally occurring isotopes, ¹⁰B and ¹¹B, with an average atomic mass of 10.812 u. Boron is 80.2 % ¹¹B, and the atomic mass of ¹¹B is 11.009 u. Calculate the mass of ¹⁰B.

The molecule drawn above has the same empirical formula as another compound "X" with a molar mass of 265.1.

Determine the molecular formula of compound "X".

A compound contains only carbon, hydrogen, and oxygen. Combustion of 15.36 mg of the compound yields 9.56 mg CO₂ and 1.80 mg H₂O. The molar mass of the compound is 120.2 g/mol. What is the molecular formula of the compound?

A compound containing only calcium, oxygen, and carbon is 45.3% Ca and 20.5% O by mass; the molar mass is 525 g/mol. What is the molecular formula of the compound?

A sample of a compound is a mixture of FNO₃and ClNO₃. The compound is analyzed in a laboratory, and the results are recorded in the table above. Calculate the mole ratio of Cl to F in the compound?

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AP Chemistry Topic 1

25 questions

According to the following reaction, how many grams of ammonia will be formed upon the complete reactions of 15.8 grams of nitrogen gas with excess hydrogen gas?

A sample of a hydrate of Na2CO3 with a mass of 550 grams was heated until all the water was removed. The sample was then weighed and found to have a mass of 300 grams. What is the formula for the hydrate?

Al2O3(l) → Al(s) + O2(g)Approximately how many liters of oxygen gas will be evolved at STP, if 25.68 grams of alumina decomposes?

The mass spectrum represented above is most consistent with which of the following elements?

An element consists of 94.93% of an isotope with mass 31.97 u, 0.76% of an isotope with mass 32.97 u, 4.29% of an isotope with mass 33.97 u, and 0.02% of an isotope with mass 35.97 u. Calculate the average atomic mass, and identify the element.

The element boron (B) has two naturally occurring isotopes, 10B and 11B, with an average atomic mass of 10.812 u. Boron is 80.2 % 11B, and the atomic mass of 11B is 11.009 u. Calculate the mass of 10B.

The molecule drawn above has the same empirical formula as another compound "X" with a molar mass of 265.1.Determine the molecular formula of compound "X".

A compound contains only carbon, hydrogen, and oxygen. Combustion of 15.36 mg of the compound yields 9.56 mg CO2 and 1.80 mg H2O. The molar mass of the compound is 120.2 g/mol. What is the molecular formula of the compound?

A compound containing only calcium, oxygen, and carbon is 45.3% Ca and 20.5% O by mass; the molar mass is 525 g/mol. What is the molecular formula of the compound?

A sample of a compound is a mixture of FNO3 and ClNO3. The compound is analyzed in a laboratory, and the results are recorded in the table above. Calculate the mole ratio of Cl to F in the compound?

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Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

A sample of a hydrate of Na₂CO₃ with a mass of 550 grams was heated until all the water was removed. The sample was then weighed and found to have a mass of 300 grams. What is the formula for the hydrate?

Al₂O₃(l) → Al(s) + O₂(g)

Approximately how many liters of oxygen gas will be evolved at STP, if 25.68 grams of alumina decomposes?

The element boron (B) has two naturally occurring isotopes, ¹⁰B and ¹¹B, with an average atomic mass of 10.812 u. Boron is 80.2 % ¹¹B, and the atomic mass of ¹¹B is 11.009 u. Calculate the mass of ¹⁰B.

The molecule drawn above has the same empirical formula as another compound "X" with a molar mass of 265.1.

Determine the molecular formula of compound "X".

A compound contains only carbon, hydrogen, and oxygen. Combustion of 15.36 mg of the compound yields 9.56 mg CO₂ and 1.80 mg H₂O. The molar mass of the compound is 120.2 g/mol. What is the molecular formula of the compound?

A sample of a compound is a mixture of FNO₃and ClNO₃. The compound is analyzed in a laboratory, and the results are recorded in the table above. Calculate the mole ratio of Cl to F in the compound?