Atomic Structure Quiz
48 Questions
0 Views

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to Lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What particles make up an atom?

  • Protons, neutrons, and positrons
  • Electrons, muons, and hadrons
  • Protons, electrons, and neutrinos
  • Protons, neutrons, and electrons (correct)

Which particle is responsible for the positive charge of the atom?

  • Neutron
  • Electron
  • Proton (correct)
  • Nucleus

What is the approximate relative mass of a neutron in atomic mass units (amu)?

  • 1.009 amu (correct)
  • 1.6750 amu
  • 0.0005 amu
  • 1.0002 amu

How does the charge of an electron compare to a proton?

<p>Electrons have a negative charge (A)</p> Signup and view all the answers

Where are electrons located in an atom?

<p>In the space around the nucleus (A)</p> Signup and view all the answers

What accounts for the mass of an atom?

<p>Protons and neutrons (C)</p> Signup and view all the answers

Which ion is not part of the isoelectronic series along with O2-, F–, Ne, Mg2+, and Al3+?

<p>Na+ (D)</p> Signup and view all the answers

What is the charge of a neutron?

<p>Neutral charge (D)</p> Signup and view all the answers

Which statement about the number of electrons in an atom is true?

<p>It is equal to the number of protons (C)</p> Signup and view all the answers

What characterizes a covalent bond?

<p>Electrons are shared between two nuclei. (B)</p> Signup and view all the answers

Which of the following pairs of atoms would most likely form a polar covalent bond?

<p>C and O (C)</p> Signup and view all the answers

How are double covalent bonds formed?

<p>By sharing two pairs of valence electrons. (C)</p> Signup and view all the answers

What typically signifies the stability of covalent bonds?

<p>High energy required to rearrange them. (D)</p> Signup and view all the answers

In which of the following statements is a characteristic of a single covalent bond?

<p>They involve the sharing of one pair of electrons. (A)</p> Signup and view all the answers

What kind of charge separation occurs in a polar covalent bond?

<p>Partial positive and partial negative charge separation occurs. (D)</p> Signup and view all the answers

Which of the following describes the general behavior of covalent bonds in living systems?

<p>They form with a limited number of different atoms. (A)</p> Signup and view all the answers

What is the primary factor that determines the strength of dipole-induced dipole interactions?

<p>Polarizability of the nonpolar molecule (A), Charge of the polar molecule (B)</p> Signup and view all the answers

Which of the following best describes London forces?

<p>Forces arising from the distortion of electron clouds (B)</p> Signup and view all the answers

What condition is necessary for an ionic bond to form between a metal and a nonmetal?

<p>Electronegativity difference must be greater than 2 (B)</p> Signup and view all the answers

How is bond dissociation energy defined?

<p>The energy required to break a bond (D)</p> Signup and view all the answers

What happens to a nonpolar molecule during interaction with a polar molecule?

<p>It is induced to become polar (D)</p> Signup and view all the answers

What characteristic of an ionic bond is affected by the size and charge of the ions involved?

<p>The strength of the attraction (B)</p> Signup and view all the answers

Which of the following describes ionic substances accurately?

<p>They require one atom to easily lose electrons and another with a high affinity for electrons (A)</p> Signup and view all the answers

What is the significance of the geometry and complexity of molecules in relation to London forces?

<p>They influence the magnitude of the force (C)</p> Signup and view all the answers

What is the primary reason ionic bonds in a cell are generally weak?

<p>The presence of water (C)</p> Signup and view all the answers

Which of the following best describes a coordinate bond?

<p>A bond where one species provides both electrons (D)</p> Signup and view all the answers

Which interaction is characterized by a dipole attracting another dipole?

<p>Dipole-dipole interaction (B)</p> Signup and view all the answers

What does the dipole moment (μ) represent in a molecule?

<p>The product of charge magnitude and distance of separation (A)</p> Signup and view all the answers

In an ion-dipole interaction, which factor does not influence the strength of the interaction?

<p>Color of the molecules involved (A)</p> Signup and view all the answers

Van der Waals forces are primarily characterized by which of the following?

<p>Weak interactions resulting from dipole interactions (D)</p> Signup and view all the answers

How is an ion-induced dipole interaction defined?

<p>Interaction between an ion and a non-polar molecule (D)</p> Signup and view all the answers

In polar molecules, what do the positive and negative poles represent?

<p>Regions of differing charge distribution (B)</p> Signup and view all the answers

What is the atomic weight of Boron based on its isotopic composition?

<p>10.8 amu (C)</p> Signup and view all the answers

Which of the following statements about isotopes is true?

<p>Isotopes of an element can have different atomic weights. (B)</p> Signup and view all the answers

Which isotope is NOT radioactive?

<p>Hydrogen (A)</p> Signup and view all the answers

From the listed isotopes of hydrogen, which one is radioactive?

<p>Tritium (D)</p> Signup and view all the answers

What decay product does Tritium produce?

<p>Helium (C)</p> Signup and view all the answers

Which of the following pairs correctly identifies the decay of Carbon-14?

<p>Carbon-14 to Nitrogen-14 (B)</p> Signup and view all the answers

What is formed when an electron is added to a neutral atom?

<p>Anion (B)</p> Signup and view all the answers

Which statement about the isotopes of Hydrogen is correct?

<p>Deuterium has one neutron. (C)</p> Signup and view all the answers

What occurs when an atom gains one or more electrons?

<p>It forms an anion. (D)</p> Signup and view all the answers

Which of the following factors contributes to an atom's electronegativity?

<p>Ionization energy (A)</p> Signup and view all the answers

How does ionization energy behave across the periodic table?

<p>It increases from the lower left to the upper right. (A)</p> Signup and view all the answers

What is the definition of electron affinity?

<p>The energy released when an electron is added to an atom. (D)</p> Signup and view all the answers

In terms of atomic structure, what does the principal quantum number (n) indicate?

<p>The size of an orbital and its energy. (A)</p> Signup and view all the answers

Which statement about angular momentum quantum number (l) is true?

<p>It represents the shape of the orbitals. (C)</p> Signup and view all the answers

What is the range of values for the magnetic quantum number (m1) when l=2?

<p>-2 to 2 (B)</p> Signup and view all the answers

Which type of element typically exhibits a high electron affinity?

<p>Nonmetals (D)</p> Signup and view all the answers

Flashcards

London Dispersion Forces

Weak intermolecular forces caused by temporary/instantaneous dipoles in molecules, arising from electron movement.

Dipole-induced dipole interaction

Interaction between a polar and nonpolar molecule, where the polar molecule induces a dipole in the nonpolar molecule.

Bond Length

Distance between the nuclei of two bonded atoms.

Bond Dissociation Energy

Energy needed to break a chemical bond.

Signup and view all the flashcards

Ionic Bonding

Bond formed by the electrostatic attraction between oppositely charged ions (cations and anions).

Signup and view all the flashcards

Ionic Compound

Compound formed by the transfer of electrons between a metal and a nonmetal.

Signup and view all the flashcards

Electronegativity

Measure of how strongly an atom attracts electrons in a chemical bond.

Signup and view all the flashcards

Cation

Positively charged ion formed by losing electrons.

Signup and view all the flashcards

Isoelectronic Series

A group of atoms or ions that have the same number of electrons.

Signup and view all the flashcards

Covalent Bonding

A type of chemical bond where atoms share electrons to achieve a stable outer shell.

Signup and view all the flashcards

What are the 6 most common atoms in living systems?

Hydrogen, carbon, nitrogen, phosphorus, oxygen, and sulfur.

Signup and view all the flashcards

Polar Covalent Bond

A covalent bond where the electrons are shared unequally, creating partial charges.

Signup and view all the flashcards

Single Covalent Bond

A bond where two atoms share one pair of electrons.

Signup and view all the flashcards

Double Covalent Bond

A bond where two atoms share two pairs of electrons.

Signup and view all the flashcards

Why are covalent bonds stable?

Because the energy required to break them is greater than available thermal energy at normal temperatures.

Signup and view all the flashcards

How do atoms in a covalent bond achieve stability?

By sharing electrons, they get a full outer shell, resembling a noble gas configuration.

Signup and view all the flashcards

Proton

A subatomic particle found in the nucleus of an atom. It carries a positive charge and has a mass of approximately 1 atomic mass unit (amu).

Signup and view all the flashcards

Electron

A subatomic particle that carries a negative charge and orbits the nucleus of an atom in a cloud-like region.

Signup and view all the flashcards

Neutron

A subatomic particle found in the nucleus of an atom. It has no charge (neutral) and has a mass of approximately 1 atomic mass unit (amu).

Signup and view all the flashcards

Atomic Nucleus

The central core of an atom, composed of protons and neutrons. It contains nearly all of the atom's mass.

Signup and view all the flashcards

Atomic Structure

The arrangement of protons, neutrons, and electrons within an atom. This arrangement determines an atom's properties and how it interacts with other atoms.

Signup and view all the flashcards

Electron Cloud

The region around the nucleus of an atom where electrons are most likely to be found. It is not a solid object but rather a probabilistic representation of electron movement.

Signup and view all the flashcards

How many electrons are in an atom?

The number of electrons in an atom is typically equal to the number of protons in its nucleus. This balances out the positive and negative charges, making the overall atom electrically neutral.

Signup and view all the flashcards

Coordinate Bond

A type of bond where both electrons involved in bonding come from one atom.

Signup and view all the flashcards

Van der Waals Forces

Weak intermolecular forces that occur due to temporary or permanent dipoles in molecules.

Signup and view all the flashcards

Dipole Moment

A measure of the separation of positive and negative charges within a molecule, essentially indicating its polarity.

Signup and view all the flashcards

Dipole-dipole Interaction

Attraction between polar molecules where the positive end of one molecule attracts the negative end of another.

Signup and view all the flashcards

Ion-dipole Interaction

Attraction between an ion (charged particle) and a polar molecule.

Signup and view all the flashcards

Ion-induced Dipole Interaction

Interaction where an ion induces a temporary dipole in a nonpolar molecule.

Signup and view all the flashcards

What makes Ion-dipole stronger than Dipole-dipole?

Ion-dipole interactions are stronger because ions have a much larger charge density than polar molecules.

Signup and view all the flashcards

How do van der Waals forces contribute to protein structure?

They stabilize the folded structure of proteins, particularly in hydrophobic regions where water is excluded.

Signup and view all the flashcards

Isotope

Atoms of the same element with the same number of protons but different numbers of neutrons. This means they have the same atomic number but different atomic masses.

Signup and view all the flashcards

Atomic Weight

The average mass of an element's atoms, taking into account the abundance of its isotopes.

Signup and view all the flashcards

Radioactive Isotope

An isotope with an unstable nucleus that decays, emitting energy or radiation until it becomes stable.

Signup and view all the flashcards

Radioactive Isotope Uses

Radioactive isotopes are used in various scientific and medical applications, such as tracing chemical processes, diagnosing diseases, and generating energy.

Signup and view all the flashcards

Forming Ions

Atoms form cations by losing electrons to achieve a stable electron configuration, while they form anions by gaining electrons to achieve a stable configuration.

Signup and view all the flashcards

Ionization Energy

The energy required to remove an electron from an atom in its gaseous state to form a positive ion. Higher values mean electrons are harder to remove.

Signup and view all the flashcards

Electron Affinity

The energy released when an electron is added to a neutral atom in its gaseous state. Higher values mean atoms readily accept electrons.

Signup and view all the flashcards

Quantum Numbers

A set of numbers that describe the properties of an electron in an atom, including its energy, shape, and spatial orientation.

Signup and view all the flashcards

Principal Quantum Number (n)

Describes the electron's energy level and the size of its orbital. Higher values indicate higher energy and larger orbitals.

Signup and view all the flashcards

Angular Momentum Quantum Number (l)

Describes the shape of an electron's orbital. Values range from 0 to n-1, with 0 representing a spherical shape.

Signup and view all the flashcards

Magnetic Quantum Number (m1)

Describes the orientation (direction in space) of an electron's orbital. Values range from -l to +l, including 0.

Signup and view all the flashcards

Study Notes

Atomic Structure

  • Atoms are the basic units of matter composed of a dense nucleus containing protons and neutrons, surrounded by electrons.
  • Protons have a positive charge, neutrons have no charge, and electrons have a negative charge.
  • The number of protons in an atom's nucleus defines the atomic number (Z).
  • The mass number (A) is the sum of protons and neutrons in an atom.
  • Isotopes are atoms of the same element with different numbers of neutrons.
  • Atoms are extremely small.

Atomic Structure: Key Terms

  • Mass number (A): Sum of protons and neutrons.
  • Atomic number (Z): Number of protons.
  • Atomic mass: Average mass of all isotopes of an element.
  • Isotopes: Atoms of the same element with different numbers of neutrons.

Atomic Structure: Isotopes

  • Isotopes have the same number of protons (and thus atomic number) but different numbers of neutrons, resulting in different mass numbers.
  • The average atomic mass listed for elements on the periodic table is an average of the different isotopes that occur naturally.

Atomic Structure: Atomic Mass

  • It's the weighted average of all naturally occurring isotopes of an element.
  • Example: Boron has two isotopes (Boron-10 and Boron-11).

Atomic Structure: Radioisotopes

  • Unstable isotopes that decay, emitting energy or particles until they become stable.
  • Used in various applications, from medical imaging to dating fossils.

Atomic Structure: Ions

  • Atoms that have lost or gained electrons, resulting in a positive or negative charge.
  • Cations are positively charged ions (loss of electrons).
  • Anions are negatively charged ions (gain of electrons).

Atomic Structure: Electronic Configuration

  • Represents the arrangement of electrons in energy levels and sublevels.
  • Electronic configuration is written e.g. 1s2 2s2 2p6 - this shows the filling pattern of the energy levels and sub-levels.
  • The periodic table can be used to predict electronic configurations.

Electronegativity

  • Measure of an atom's ability to attract shared electrons in a chemical bond.
  • Higher electronegativity means stronger attraction for electrons.
  • Trend in the periodic table: Electronegativity generally increases across a period and decreases down a group.

Chemical Bonding

  • Forces that hold atoms together in molecules or compounds.
  • Covalent bonds: Sharing of electrons between atoms.
  • Ionic bonds: Transfer of electrons to form oppositely charged ions which attract.
  • Polar bonds: Unequal sharing of electrons in a covalent bond, creating partial charges.
  • Non-polar bonds: Equal sharing of electrons in a covalent bond.
  • Hydrogen bonds: Weak forces between a hydrogen atom bonded to a highly electronegative atom and another electronegative atom.
  • Van der Waals forces: Weak attractive forces between molecules; momentary instantaneous dipoles.

Types of Bonds

  • Covalent Bonds: Electrons are shared between atoms resulting in a molecule
  • Ionic Bonds: Electrons are transferred from one atom to another resulting in ions.
  • Metallic Bonds: Electrons are shared among many atoms.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Quiz Team

Related Documents

CSIR NET Unit 1(A) Notes - Structure of Atoms, Molecules & Chemical Bonds PDF

Description

Test your knowledge on the basics of atomic structure, including definitions of protons, neutrons, electrons, and isotopes. This quiz covers key terms such as atomic number and mass number, helping you grasp fundamental concepts in chemistry. Perfect for students learning about the composition of matter.

More Like This

Química: Átomos y Estructura Electrónica
6 questions

Química: Átomos y Estructura Electrónica

ToughStanza avatar
ToughStanza
Counting Protons, Neutrons, and Electrons
5 questions

Counting Protons, Neutrons, and Electrons

CarefreeMeerkat avatar
CarefreeMeerkat
Atomic Structure Basics
5 questions

Atomic Structure Basics

EvocativeSphene avatar
EvocativeSphene
Atomic Structure and Nucleon Numbers
41 questions

Atomic Structure and Nucleon Numbers

AgreeableIntegral4204 avatar
AgreeableIntegral4204
Use Quizgecko on...
Browser
Open
Browser
Browser