CLASS 7 CHEMISTRY: ATOMIC STRUCTURE

What is the basic unit of matter?

What particles are present in the nucleus of an atom?

What is the charge of an electron?

What is the atomic number of an element equal to?

Which of the following is a diatomic molecule?

What is the mass number of an atom?

What is the name of a charged atom?

Who discovered the electron?

In the Modern Periodic Table, what do group numbers signify?

What is a radical?

What is the term for the combining capacity of an element?

Which subatomic particle has no charge?

What does a chemical formula represent?

What is the purpose of balancing a chemical equation?

What are the horizontal rows in the Modern Periodic Table called?

According to Dalton's atomic theory, are atoms destructible or indestructible?

What did Rutherford's gold foil experiment discover?

Who discovered neutrons?

What is a molecule?

What term describes the number of atoms present in a molecule of an element?

If an element has a variable valency, what does this indicate about its combining capacity?

Which of the following statements accurately describes the relationship between radicals and chemical reactions?

How does the Modern Periodic Table arrange elements?

Which of the following describes the significance of the group number in the Modern Periodic Table?

What information does a chemical formula provide about a compound?

Why is it necessary to balance a chemical equation?

According to the Modern Atomic Theory, how do atoms of the same element compare?

Which subatomic particle was discovered by James Chadwick?

How would you classify oxygen ($O_2$)?

Which best describes a radical?

An element is known to form a divalent cation. What does this imply about the element's valency?

What principle underlies the balancing of chemical equations?

What is the significance of periods in the Modern Periodic Table?

What did Rutherford's model of the atom propose regarding the location of positive charge?

How does the modern atomic theory differ from Dalton's atomic theory regarding the indivisibility of atoms?

Consider a neutral atom with an atomic number of 16 and a mass number of 32. How many neutrons does it possess?

What does the term 'atomicity' refer to?

Elements are arranged in the periodic table in periods and groups. What is a key difference between elements in the same group versus elements in the same period?

Given a compound with a chemical formula $XY_2$, if X is known to be a divalent cation, what is the likely charge of the $Y$ ion to maintain charge neutrality?

How is a 'cation' defined in terms of electron gain or loss?

An element exhibits two valencies, +2 and +3. Which statement best explains how these variable valencies arise based on electronic structure?

Consider a newly synthesized molecule with the formula $X_2Y_3$. If element Y is known to readily form anions with a -2 charge, what is the likely charge of element X to ensure the molecule is neutral?

Given two isotopes of the same element, which of the following properties will always be identical?

A neutral atom has an electron configuration of $1s^22s^22p^63s^23p^5$. Which statement accurately describes the ion this atom is most likely to form??

How does the behavior of a radical in a chemical reaction differ from that of a typical ion or molecule?

In mass spectrometry, isotopes of an element are separated based on their mass-to-charge ratio. For two isotopes of chlorine, $^{35}Cl$ and $^{37}Cl$, which statement accurately predicts their behavior in a mass spectrometer?

Consider a compound formed between a Group 2 element (alkaline earth metal) and a Group 16 element (chalcogen). How would the bond formed between these elements be classified, and what properties would the resulting compound likely exhibit?

If a newly discovered element is found to have similar chemical properties to oxygen and sulfur, to which group in the Modern Periodic Table would this element likely belong?

An unknown gas is found to consist of diatomic molecules. Under extreme conditions, these molecules break apart, forming highly reactive single atoms. How does the behavior of these single atoms differ from that of the original diatomic molecules?

How does the concept of 'atomicity' relate to the physical state (gas, liquid, or solid) of an element at room temperature?

An atom is the basic unit of matter.

Molecules can only be formed from different elements.

A radical is always a positively charged ion.

Atomicity refers to the number of protons in a molecule.

The positive part of a compound is called the acidic radical.

Valency is the combining capacity of an element.

Valency can be a fraction.

Some elements can have more than one valency.

A chemical formula only shows the types of elements in a substance.

A chemical equation uses symbols and formulas to represent a chemical reaction.

A balanced equation violates the law of conservation of mass.

The number of atoms of reactants is less than the number of atoms of products.

The modern periodic table arranges elemets in increasing order of atomic mass.

Periods in the Modern Periodic Table are arranged in vertical columns.

The group number in the Modern Periodic Table signifies the number of electrons in the outermost shell of an atom.

A molecule is formed when two or more atoms of the same element combine, but not when atoms of different elements combine.

A radical always consists of a single atom with a positive charge.

Atomicity refers to the number of different elements present in a molecule.

In a compound, the basic radical is the negative part, while the acidic radical is the positive part.

The valency of an element can be a fraction, representing its combining capacity.

Elements with variable valency always exhibit only two different valency states.

A chemical formula only indicates the types of elements present in a compound, not the number of atoms of each element.

A balanced chemical equation violates the law of conservation of mass by showing unequal numbers of atoms on both sides.

The law of conservation of mass states that the total mass of reactants is less than the total mass of products in a chemical reaction.

In the Modern Periodic Table, periods are vertical columns, while groups are horizontal rows.

The group number in the Modern Periodic Table signifies the number of neutrons in the outer shell of an atom.

Dalton’s atomic theory stated that atoms are divisible and consist of protons, electrons, and neutrons.

Rutherford's gold foil experiment led to the discovery of electrons.

Neutrons have a positive charge equal in magnitude to that of a proton.

An ______ is the basic unit of matter and the smallest particle of an element.

A ______ is the smallest particle of a substance capable of independent existence.

A ______ is a single atom or group of atoms that behaves as a single unit with a charge.

______ is the number of atoms present in a molecule of an element.

A ______ is composed of a positive part (basic radical) and a negative part (acidic radical).

The combining capacity of an element is also known as its ______.

Elements that exhibit more than one valency are said to have ______ valency.

A ______ formula is a representation of a substance using symbols.

A chemical ______ uses symbols and formulas to represent reactants and products in a chemical reaction.

A balanced equation complies with the law of chemical ______ of mass.

The modern periodic table arranges elements in increasing order of ______ numbers.

In the modern periodic table, horizontal rows are called ______ and vertical columns are called groups.

The group number in the periodic table signifies the number of ______ in the outer shell of an atom.

______ are built up of three sub-atomic particles: protons, neutrons, and electrons.

The ______ of an element depends upon the atoms constituting it.

A/an ______ is the smallest particle of an element that retains the properties of that element.

According to Dalton's Atomic Theory, all matter is made up of indivisible particles called ______. Each element consists of identical atoms.

The law of ______ states that atoms cannot be created or destroyed in chemical reactions.

An atom contains a central ______ and ______ moving around in specific orbits.

The three subatomic particles that constitutes an atom are ______ (positively charged), ______ (neutral charge), and ______ (negatively charged).

[Blank] were discovered by J.J. Thomson in 1897 through the cathode ray tube experiment.

The ______ was discovered by Ernest Rutherford in 1911, through his gold foil experiment.

[Blank] were discovered by James Chadwick in 1932.

In the nucleus of an atom, ______ have a positive charge (+1) and a mass of 1 unit, while ______ have no charge (neutral) and a mass of 1 unit.

The ______ contains protons and neutrons, giving the atom most of its mass.

The concept that electrons are arranged in different orbits or energy levels around the nucleus is known as the ______.

According to Niels Bohr, electrons revolve around the nucleus in fixed orbits or energy levels, each having a specific energy; the energy levels are numbered as K, L, M, N, etc., from the nucleus outward, each level has a ______ number of electrons it can hold.

The ______ is the number of protons in the nucleus of an atom and is also equal to the number of electrons in a neutral atom.

The ______ is the sum of protons and neutrons in the nucleus of an atom.

[Blank] are atoms of the same element with the same number of protons but different numbers of neutrons, leading to different mass numbers.

What particles are found in the nucleus of an atom?

What is the name for the outermost electron shell of an atom?

What is the number of atoms present in a molecule called?

What is a molecule composed of two atoms called?

What is the name given to atoms of the same element with different numbers of neutrons?

What is a charged atom or molecule called?

If an atom loses electrons, does it form a positive or negative ion?

What is the horizontal row in the periodic table called?

What is the vertical column in the periodic table called?

What is a combination of symbols that represent a compound called?

What is the sum of protons and neutrons in an atom's nucleus?

What number is used to organizes elements in the modern periodic table?

What is a group of atoms behaving as a single unit with a charge called?

Explain how the properties of an element are related to the atoms that constitute it. Provide an example.

Compare and contrast a molecule of an element with a molecule of a compound, giving an example of each.

Define what a radical is in chemistry, and provide an example, explaining why it is classified as a radical.

Given that a molecule of ozone ($O_3$) contains three oxygen atoms, what term is used to describe its atomicity, and what does this term mean?

Explain how the concepts of 'basic radical' and 'acidic radical' are used to understand the composition of a compound. Provide an example using NaCl.

Describe how the valency of an element determines its combining capacity, and give an example of an element with a valency of 2.

What is variable valency, and why do some elements exhibit this property? Give an example of an element with variable valency.

How does a chemical formula represent the composition of a substance? Give an example using water ($H_2O$).

Why is it important to balance a chemical equation? State the law that necessitates balancing, and explain its relevance.

Briefly describe how the modern periodic table is organized and what single factor primarily determines the arrangement of elements.

Describe the significance of the group number in the modern periodic table relating to the electronic structure and chemical properties of elements.

How did J.J. Thomson's experiments contribute to our understanding of atomic structure, and what specific subatomic particle did he discover?

Explain how Rutherford’s gold foil experiment changed the understanding of atomic structure, and what key feature of the atom did he discover?

Briefly explain how isotopes of an element differ from each other, and what remains the same between them. Provide an example using carbon isotopes.

Explain the octet rule and its significance in chemical bonding. How do atoms typically achieve an octet in their outermost shell?

How does the concept of variable valency challenge the earlier, simpler models of chemical bonding, and what implications does it have for predicting the formulas of chemical compounds?

Explain how Rutherford's gold foil experiment led to a departure from the plum pudding model of the atom and what key observations necessitated this change?

Describe how the concept of 'atomicity' relates to the physical state (e.g., gas, liquid, solid) of an element at room temperature and pressure, providing specific examples.

Discuss the limitations of Dalton's atomic theory in light of modern discoveries regarding subatomic particles and isotopes.

Explain how the octet rule, while useful, can sometimes fail to predict the stability of molecules, especially those involving elements beyond the second period.

How does the concept of 'radical' differ from that of a 'molecule,' and where might radicals play a crucial role in chemical reactions differently from stable molecules?

If an electrically neutral atom loses two electrons, what type of ion is formed, and how does its radius typically compare to that of the original neutral atom? Explain the underlying reasons for this change in radius.

Describe the relationship between the number of valence electrons an atom possesses and its placement in the modern periodic table (specifically, its group number). How does this relationship reflect the chemical properties of elements within the same group?

Explain how isotopes of an element can have different physical properties (such as density or rate of diffusion) despite having nearly identical chemical properties. Provide a rationale for this difference.

How does the law of conservation of mass apply to balancing chemical equations, and what does it imply about the number and type of atoms present on both sides of a balanced equation?