Atomic structure
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1.Which subatomic particle has a positive charge?
Easy- AProton
- BNeutron
- CElectron
- DIon
2.What is the charge of a neutron?
Easy- APositive
- BNegative
- CNeutral (no charge)
- DDepends on the element
3.The nucleus of an atom contains protons and neutrons.
EasyTrue or false?
4.Which two subatomic particles have approximately the same mass?
Easy- AProton and electron
- BNeutron and electron
- CProton and neutron
- DElectron and ion
5.Which of the following statements about isotopes are true? (Select all that apply)
Medium- AIsotopes have the same number of protons.
- BIsotopes have the same number of neutrons.
- CIsotopes have different atomic masses.
- DIsotopes have different chemical properties.
- EIsotopes are atoms of the same element.
6.Arrange the following in order of increasing mass: electron, proton, neutron.
Easy- Electron
- Proton
- Neutron
7.Dalton's law of multiple proportions suggests that elements combine in ratios of small whole numbers. Which of the following pairs of compounds best illustrates this law?
Medium- AH2O and H2O2
- BNaCl and KCl
- CCO2 and SO2
- DCH4 and C2H6
8.Which statement best describes the distribution of mass in an atom?
Easy- AMass is evenly distributed throughout the atom.
- BMost of the mass is in the electron cloud.
- CMore than 99.94% of the mass is in the nucleus.
- DProtons and electrons contribute equally to the mass.
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9.Match each subatomic particle with its relative charge.
Easy- Proton
- Neutron
- Electron
- +1
- 0
10.Arrange the following particles in order of increasing mass (lightest to heaviest).
Easy- Electron
- Proton
- Neutron
11.Which of the following statements about atoms are true? (Select all that apply)
Easy- AThe nucleus contains protons and neutrons.
- BElectrons are found in shells around the nucleus.
- CThe atom is mostly empty space.
- DProtons and electrons have equal mass.
12.An atom that has gained an electron is called a cation.
EasyTrue or false?
13.In Dalton's law of multiple proportions, the ratio of oxygen masses combining with a fixed mass of tin in grey tin oxide and white tin oxide is 1:2. What is the ratio of oxygen atoms per tin atom in these two compounds?
Hard- A1:1 and 1:2
- B1:2 and 1:1
- C1:1 and 2:1
- D2:1 and 1:1
14.The diagram shows a Bohr model of a sodium atom. How many electrons are in the outermost shell?
Easy- A1
- B2
- C8
- D11
15.Which of the following are correct statements about the distribution of mass and charge in an atom? (Select all that apply)
Medium- AMore than 99% of the atom's mass is in the nucleus.
- BThe nucleus is positively charged.
- CElectrons contribute most of the atom's mass.
- DThe atom is electrically neutral if protons equal electrons.
16.Match each historical figure or concept with their contribution to atomic theory.
Medium- John Dalton
- Electron discovery
- Nucleus discovery
- Law of multiple proportions
- Plum pudding model
- Rutherford gold foil experiment
17.Arrange the following substances in order of increasing number of oxygen atoms per nitrogen atom: N2O, NO, NO2.
Medium- N2O
- NO
- NO2
18.A sample of tin oxide is found to contain 88.1% tin and 11.9% oxygen by mass. Using the law of multiple proportions, what is the likely formula of this oxide?
Hard- ASnO
- BSnO2
- CSn2O3
- DSnO3
19.Nitrous oxide (N2O) contains 63.3% nitrogen and 36.7% oxygen. Nitric oxide (NO) contains 44.05% nitrogen and 55.95% oxygen. What is the ratio of oxygen masses combining with a fixed mass of nitrogen in N2O : NO?
Hard- A1:2
- B2:1
- C1:4
- D4:1
20.Which of the following statements about Dalton's law of multiple proportions are correct? (Select all that apply)
Medium- AIt applies to compounds containing the same two elements.
- BIt states that the masses of one element that combine with a fixed mass of another element are in ratios of small whole numbers.
- CIt was used to determine atomic masses.
- DIt disproves the existence of isotopes.
21.In the Bohr model of a sodium atom (atomic number 11), how many electrons are in the second shell?
Easy- A2
- B8
- C1
- D11
22.The diagram shows a Bohr model of a sodium atom. Which part of the atom contains most of its mass?
Easy- AThe nucleus
- BThe electron shells
- CThe area outside the nucleus
- DThe first shell
23.Match each compound with its formula based on the law of multiple proportions examples given in the source.
Medium- Grey tin oxide
- White tin oxide
- Nitrous oxide
- SnO
- SnO2
- N2O
- NO
- NO2
24.An atom with more protons than electrons is a negative ion.
EasyTrue or false?
25.A sample of iron(II) oxide (FeO) is found to contain 77.7% iron by mass. What is the approximate percentage of iron in iron(III) oxide (Fe2O3)? (Atomic masses: Fe = 55.8, O = 16.0)
Challenge- A70.0%
- B72.4%
- C69.9%
- D77.7%
26.Arrange the following compounds in order of increasing oxygen content per nitrogen atom (lowest to highest): N2O, NO, NO2.
Easy- N2O
- NO
- NO2
27.In an experiment to determine the composition of tin oxides, a student heats a known mass of tin in air and measures the mass of the product. The grey oxide contains 88.1% tin and 11.9% oxygen. In a separate experiment, the white oxide is found to contain 78.7% tin and 21.3% oxygen. Which of the following ratios of oxygen mass per 100 g of tin best supports Dalton's law of multiple proportions for these two oxides?
Hard- A1:2
- B2:1
- C1:3
- D3:1
28.Match each tin oxide to its formula based on the law of multiple proportions data: grey oxide (88.1% Sn, 11.9% O) and white oxide (78.7% Sn, 21.3% O).
Medium- Grey oxide
- White oxide
- SnO
- SnO2
- Sn2O3
29.Arrange the following nitrogen oxides in order of increasing oxygen content per fixed mass of nitrogen (lowest to highest): N2O, NO, NO2.
Easy- N2O
- NO
- NO2
30.In Dalton's law of multiple proportions, the ratio of oxygen masses combining with a fixed mass of tin in grey tin oxide and white tin oxide is 2:1.
MediumTrue or false?
31.A student performs an experiment to determine the formula of an oxide of nitrogen. They react 14.0 g of nitrogen with excess oxygen and obtain 30.0 g of the oxide. Which of the following is the most likely formula of the oxide? (Atomic masses: N = 14, O = 16)
Medium- ANO
- BN2O
- CNO2
- DN2O3
32.Which subatomic particle has no charge?
Easy- Aproton
- Bneutron
- Celectron
- Dion
33.What is the approximate relative mass of an electron compared to a proton?
Easy- A1/1836
- B1/100
- Cequal
- D1836 times larger
34.The nucleus of an atom contains protons, neutrons, and electrons.
EasyTrue or false?
35.Which of the following best describes the distribution of mass in an atom?
Easy- AMass is evenly distributed throughout the atom.
- BMost of the mass is in the nucleus.
- CMost of the mass is in the electron cloud.
- DProtons and electrons contribute equally to the mass.
36.Isotopes of an element have the same number of protons but different numbers of neutrons.
EasyTrue or false?
37.Arrange the following particles in order of increasing mass (lightest to heaviest):
Easy- electron
- proton
- neutron
38.Which of the following statements about ions are correct? (Select all that apply)
Medium- AA cation has a positive charge.
- BAn anion has more electrons than protons.
- CA neutral atom has equal numbers of protons and electrons.
- DIons are formed only by gaining electrons.
39.The diagram shows a Bohr model of a sodium atom. The particle labelled 'X' in the nucleus is a neutron.
EasyTrue or false?
40.Arrange the following in order of increasing mass (lightest to heaviest): proton, neutron, electron.
Easy- proton
- neutron
- electron
41.Complete the sentence:
EasyAn atom with the same number of protons but a different number of neutrons is called an ____.
42.An atom has 11 protons and 12 neutrons. What is its atomic number?
Easy43.What is the term for a charged atom?
Easy44.An atom of carbon has 6 protons and 6 neutrons. What is its mass number?
Easy45.Complete the sentence about isotopes.
EasyIsotopes of the same element have the same number of ____ but different numbers of ____.
46.In an experiment, a sample of iron oxide is 78.1% iron and 21.9% oxygen by mass. Calculate the mass of oxygen combined with 100 g of iron. Give your answer to one decimal place.
Medium47.Refer to the diagram of a sodium atom. Complete the sentence: The particle labelled 'X' in the nucleus is a ____.
EasyThe particle labelled 'X' in the nucleus is a ____.
48.What is the term for atoms of the same element that have different numbers of neutrons?
Easy49.A tin oxide sample is 88.1% tin and 11.9% oxygen by mass. Calculate the mass of oxygen (in g) that combines with 100 g of tin. Give your answer to one decimal place.
Medium50.Complete the sentence about atomic structure.
EasyThe three subatomic particles are the ____, ____, and ____.
51.Fill in the blanks to complete the sentence about isotopes.
EasyAtoms of the same element with different numbers of neutrons are called ____. They have the same number of ____ but different ____ numbers.
52.What is the atomic number of an atom that has 11 protons?
Easy53.Explain how the discovery of the electron led to the development of the plum pudding model of the atom.
Medium54.Explain how the law of multiple proportions provided evidence for the existence of atoms.
Hard55.An atom has 11 protons and 12 neutrons. What is its atomic number?
Easy- A13
- B10
- C12
- D11
56.An atom of carbon has 6 protons and 6 neutrons. What is its mass number?
Easy- A12
- B14
- C13
- D11
57.In an experiment, a sample of iron oxide is 78.1% iron and 21.9% oxygen by mass. Calculate the mass of oxygen combined with 100 g of iron. Give your answer to one decimal place.
Medium- A34 g
- B25 g
- C28 g
- D31 g
58.A tin oxide sample is 88.1% tin and 11.9% oxygen by mass. Calculate the mass of oxygen (in g) that combines with 100 g of tin. Give your answer to one decimal place.
Medium- A12.5 g
- B13.5 g
- C15.5 g
- D14.5 g
字卡
What are the three subatomic particles that make up an atom?
Protons, neutrons, and electrons.
What is the charge and relative mass of a proton?
Proton: positive charge (+1), relative mass of 1 atomic mass unit.
What is the charge and relative mass of a neutron?
Neutron: no charge (0), relative mass of 1 atomic mass unit.
What is the charge and relative mass of an electron?
Electron: negative charge (-1), relative mass approximately 1/1836 of a proton (essentially negligible).
Where is most of an atom's mass located?
More than 99.94% of an atom's mass is in the nucleus.
What is the nucleus of an atom composed of?
The nucleus is composed of protons and neutrons (except hydrogen-1, which has only a proton).
What holds the protons and neutrons together in the nucleus?
The nuclear force, which is stronger than the electromagnetic repulsion between protons.
What determines the identity of an element?
The number of protons in the atom. For example, any atom with 11 protons is sodium.
What are isotopes?
Atoms of the same element (same number of protons) but with different numbers of neutrons.
What is an ion?
An atom that has gained or lost electrons, giving it a net electric charge.
What is a cation?
A positively charged ion, formed when an atom loses electrons (more protons than electrons).
What is an anion?
A negatively charged ion, formed when an atom gains electrons (more electrons than protons).
Why are atoms electrically neutral under normal conditions?
Because they have equal numbers of protons and electrons, balancing positive and negative charges.
What force binds electrons to the nucleus?
The electromagnetic force: opposite charges attract (positive nucleus attracts negative electrons).
What is the approximate size of an atom?
Around 100 picometers (1 × 10⁻¹⁰ m) in diameter.
Why can't atoms be seen with conventional microscopes?
Atoms are smaller than the shortest wavelength of visible light, so they cannot be resolved by light microscopes.
What is the origin of the word 'atom'?
From the ancient Greek word 'atomos', meaning 'uncuttable'.
How did John Dalton contribute to atomic theory?
He provided experimental evidence that matter is composed of discrete units (atoms) and formulated the law of multiple proportions.
State the law of multiple proportions as discovered by Dalton.
When two elements form more than one compound, the masses of one element that combine with a fixed mass of the other are in ratios of small whole numbers.
Give an example of the law of multiple proportions using tin oxides.
In grey tin oxide (SnO), 100 g of tin combines with about 13.5 g of oxygen; in white tin oxide (SnO₂), 100 g of tin combines with about 27 g of oxygen. The oxygen masses are in a 1:2 ratio.
What is the formula of iron(II) oxide and iron(III) oxide?
Iron(II) oxide is FeO; iron(III) oxide is Fe₂O₃.
What are the formulas for nitrous oxide, nitric oxide, and nitrogen dioxide?
Nitrous oxide: N₂O; nitric oxide: NO; nitrogen dioxide: NO₂.
What happens when the repelling electromagnetic force in the nucleus becomes stronger than the nuclear force?
The nucleus can split (nuclear decay), leaving behind different elements.