Atomic Structure and Periodic Table Concepts

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Questions and Answers

What is the smallest part of an element that can exist?

Compound

Mixture

Molecule

Atom (correct)

Mixtures are formed through chemical reactions between elements.

False

Name three physical processes that can separate mixtures.

filtration, crystallisation, distillation

Compounds contain two or more elements chemically combined in ______ proportions.

fixed Signup and view all the answers

Match the following terms with their descriptions:

Atom = Smallest part of an element Compound = Elements chemically combined Mixture = Elements or compounds not chemically combined Chemical reaction = Formation of new substances, energy change Signup and view all the answers

Which of the following best represents a compound?

HCl Signup and view all the answers

Chemical reactions can separate compounds into elements.

True Signup and view all the answers

What type of process is chromatography used for?

separating mixtures Signup and view all the answers

What is the relative charge of a neutron?

0 Signup and view all the answers

An atom contains more mass in its nucleus than the rest of the atom.

True Signup and view all the answers

What is the mass number?

The sum of the protons and neutrons in an atom. Signup and view all the answers

The relative atomic mass is an average value that considers the abundance of the __________ of the element.

isotopes Signup and view all the answers

Match the following particles with their relative mass:

Proton = 1 Neutron = 1 Electron = Very small Signup and view all the answers

How many electrons are there in a neutral atom of an element if it has 6 protons?

6 Signup and view all the answers

Carbon-14 and Carbon-12 have the same number of protons.

True Signup and view all the answers

What is the approximate radius of an atom in nanometers?

0.1 nm Signup and view all the answers

Which model of the atom describes it as a ball of positive charge with negative electrons embedded in it?

Plum pudding model Signup and view all the answers

The early concept of atoms was that they could be divided into smaller particles.

False Signup and view all the answers

Who suggested that electrons orbit the nucleus at specific distances?

Neil Bohr Signup and view all the answers

The ______ particle scattering experiment showed that the mass of an atom is concentrated at its nucleus.

alpha Signup and view all the answers

Match the subatomic particles with their charges:

Proton = Positive charge Electron = Negative charge Neutron = No charge Signup and view all the answers

What experimentally proven particle was discovered by James Chadwick?

Neutron Signup and view all the answers

All atoms of a particular element have the same number of neutrons.

False Signup and view all the answers

What is the atomic number of an element?

The number of protons in an atom of that element. Signup and view all the answers

Study Notes

Atomic Structure and the Periodic Table

Atoms are the fundamental building blocks of all matter.
Atoms are the smallest part of an element that can exist.
Chemical symbols represent atoms (e.g., Na for sodium).
Elements form compounds through chemical reactions.
Chemical reactions involve a change in energy.
Compounds consist of two or more elements combined in fixed ratios.
Compounds are represented by formulae (e.g., HCl for hydrogen chloride).
Mixtures comprise two or more elements or compounds not chemically bonded.
Mixture components retain their properties.
Mixtures can be separated using physical processes (e.g., filtration, distillation).

Development of the Atomic Model

Early models viewed atoms as indivisible spheres.
The discovery of the electron led to the plum pudding model.
The plum pudding model depicted the atom as a sphere of positive charge with embedded negative electrons.
The alpha particle scattering experiment revealed the nucleus.
The nucleus is a dense, positively charged core at the center of the atom.
Most of the atom's mass is concentrated in the nucleus.
Electrons orbit the nucleus at specific energy levels (Bohr model).

Subatomic Particles

Protons have a positive charge (+1).
Neutrons have no charge (0).
Electrons have a negative charge (-1).
An atom is electrically neutral (protons = electrons).
Atomic number is the number of protons.
Mass number is the sum of protons and neutrons.
Isotopes are atoms of the same element with different neutron numbers.

Relative Atomic Mass

Relative atomic mass is the average mass of an atom of an element relative to 1/12 the mass of a carbon-12 atom.
It takes into account the abundance of isotopes.
Calculate relative atomic mass using the formula: ((isotope 1 mass x abundance) + (isotope 2 mass x abundance)) ÷ 100

Electronic Structure

Electrons fill the lowest energy levels first (closest to the nucleus).
Electronic structure describes the arrangement of electrons in different energy levels (shells).
For example, sodium's electronic structure is 2, 8, 1.

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Description

Test your knowledge on atomic structure and the periodic table. This quiz covers the fundamental concepts of atoms, elements, compounds, and mixtures, along with the historical development of atomic models. Assess your understanding of chemical symbols, reactions, and separation techniques.