p.3
Understanding Atoms and Elements
What are the main components of an atom?
Protons, neutrons, and electrons.
p.6
Isotopes and Their Applications
Do isotopes have identical chemical properties?
Yes, but they have different physical properties such as mass and density.
p.2
Modern Schrödinger Quantum Mechanical Model
What significant confirmation was made using STMs?
That atoms are indeed spherical.
p.5
Isotopes and Their Applications
What is the significance of studying isotopes in climate change research?
Isotopes help determine past temperatures by analyzing the ratio of oxygen isotopes in ice cores.
p.2
Atomic Theory and Historical Perspectives
What is a scientific model?
A tool used by scientists to explain something they cannot see directly.
p.2
Atomic Theory and Historical Perspectives
What did Dalton propose about atoms?
That all matter is made up of tiny spherical particles that are indivisible and indestructible.
p.2
Modern Schrödinger Quantum Mechanical Model
How do scanning tunneling microscopes (STMs) work?
They use a sharp metal tip to detect atoms by measuring height differences on a crystal's surface.
p.4
Understanding Atoms and Elements
What does the mass number represent?
The mass number represents the total number of protons and neutrons in the nucleus.
p.8
Chemical Symbols and Notation
What is the chemical symbol of an element composed of?
One or two letters, with the first letter capitalized and the second letter lowercase.
p.1
Understanding Atoms and Elements
What will you review at the beginning of the chapter?
Your understanding of atoms and elements.
p.2
Understanding Atoms and Elements
What are elements?
Materials that contain just one type of atom.
p.8
Understanding Atoms and Elements
What are atoms composed of?
A small, positively charged nucleus surrounded by a negatively charged cloud of electrons.
p.8
Subatomic Particles: Protons, Neutrons, and Electrons
What are the charges of protons, neutrons, and electrons?
Protons have a positive charge, electrons have a negative charge, and neutrons have no charge.
p.4
Chemical Symbols and Notation
Why do some chemical symbols not correspond to the name of the element?
Some chemical symbols are derived from the Latin or Greek names of the elements.
p.1
Critical and Endangered Elements
What are critical elements mentioned in the chapter?
Helium, phosphorus, rare-earth elements, and post-transition metals.
p.3
Subatomic Particles: Protons, Neutrons, and Electrons
How much smaller is an electron compared to a proton or neutron?
Approximately 1/800 times smaller.
p.4
Understanding Atoms and Elements
What is the atomic number represented by?
The atomic number is represented by the symbol Z and is equal to the number of protons in the nucleus.
p.8
Isotopes and Their Applications
What are isotopes?
Atoms with the same atomic number but different mass numbers, meaning they have the same number of protons but different numbers of neutrons.
p.1
Modern Schrödinger Quantum Mechanical Model
What model will you learn about regarding electron behavior in atoms?
The modern Schrödinger quantum mechanical model.
p.1
Isotopes and Their Applications
What definitions will you learn regarding isotopes and ions?
Definitions including atomic number, mass number, and the number of protons, neutrons, and electrons.
p.7
Ions and Their Formation
What happens to an atom that loses electrons?
It becomes positively charged.
p.4
Atomic Theory and Historical Perspectives
What did Rutherford's gold foil experiment demonstrate about atoms?
Atoms are mostly empty space with a small, extremely dense nucleus.
p.5
Isotopes and Their Applications
What do higher amounts of oxygen-18 in ice cores indicate?
Higher temperatures when the water originally fell as rain.
p.8
Isotopes and Their Applications
How can you determine the number of neutrons in an atom?
By subtracting the atomic number (number of protons) from the mass number.
p.7
Ions and Their Formation
What are ions?
Atoms that have lost or gained one or more electrons.
p.6
Isotopes and Their Applications
What effect did nuclear weapons testing have on carbon-14 levels?
It caused a spike in carbon-14 in the atmosphere.
p.5
Subatomic Particles: Protons, Neutrons, and Electrons
What does the atomic number (Z) indicate in an atom?
The number of protons and electrons in the atom.
p.5
Chemical Symbols and Notation
What is nuclide notation?
A standard way of representing an atom showing its atomic number and mass number.
p.4
Understanding Atoms and Elements
How many elements have been discovered by scientists?
Scientists have discovered 118 different elements.
p.5
Subatomic Particles: Protons, Neutrons, and Electrons
What is the mass number (A) in relation to protons and neutrons?
The mass number is the sum of protons and neutrons in an atom.
p.6
Isotopes and Their Applications
How do isotopes of the same element differ?
They have the same number of protons but different numbers of neutrons.
p.6
Isotopes and Their Applications
What are the mass numbers of the isotopes of carbon?
Carbon-12, Carbon-13, and Carbon-14.
p.3
Subatomic Particles: Protons, Neutrons, and Electrons
What is the nucleus of an atom primarily made of?
Protons and neutrons, collectively called nucleons.
p.8
Subatomic Particles: Protons, Neutrons, and Electrons
What determines the mass of an atom?
The mass of the nucleus, which is made up of protons and neutrons.
p.3
Understanding Atoms and Elements
What is the size comparison between an atom and its nucleus?
The nucleus is approximately 10,000-100,000 times smaller than the atom.
p.6
Isotopes and Their Applications
What are isotopes?
Atoms with the same atomic number but different mass numbers.
p.2
Atomic Theory and Historical Perspectives
What do scientists now know about atoms compared to Dalton's theory?
Atoms are not indivisible or indestructible; they are made up of smaller subatomic particles.
p.6
Isotopes and Their Applications
What does it mean if an isotope is radioactive?
Its nucleus is unstable and will break down spontaneously by emitting radiation.
p.4
Chemical Symbols and Notation
What is the chemical symbol for sodium?
The chemical symbol for sodium is Na.
p.7
Ions and Their Formation
What happens to an atom that gains electrons?
It becomes negatively charged.
p.7
Subatomic Particles: Protons, Neutrons, and Electrons
How many neutrons are in the ion Mg²⁺?
13 (mass number 25 - atomic number 12).
p.3
Subatomic Particles: Protons, Neutrons, and Electrons
What happens when you rub a rubber balloon on a woollen jumper?
Electrons are transferred to the balloon, giving it a negative charge.
p.8
Isotopes and Their Applications
What is the significance of Yttrium-90?
It is used for the treatment of cancer, particularly non-Hodgkin lymphoma and liver cancer.
p.2
Understanding Atoms and Elements
What are compounds?
Materials that contain different types of atoms in fixed ratios.
p.4
Subatomic Particles: Protons, Neutrons, and Electrons
What is the charge on an electron compared to a proton?
The charge on an electron is equal but opposite to the charge on a proton.
p.7
Subatomic Particles: Protons, Neutrons, and Electrons
How do you calculate the number of neutrons in an ion?
Mass number - atomic number.
p.8
Subatomic Particles: Protons, Neutrons, and Electrons
How much smaller are electrons compared to protons and neutrons?
Electrons are approximately 1800 times smaller.
p.4
Understanding Atoms and Elements
What is the significance of the number of protons in an atom?
The number of protons determines the identity of the element.
p.6
Isotopes and Their Applications
What are the names of the three isotopes of hydrogen?
Protium, Deuterium, and Tritium.
p.2
Modern Schrödinger Quantum Mechanical Model
What type of microscope was developed to view atoms?
Scanning tunneling microscope (STM).
p.5
Subatomic Particles: Protons, Neutrons, and Electrons
For an aluminum atom with atomic number 13, how many protons and electrons does it have?
It has 13 protons and 13 electrons.
p.3
Subatomic Particles: Protons, Neutrons, and Electrons
What phenomenon explains why electrons are bound to the nucleus?
Electrostatic attraction.
p.8
Ions and Their Formation
What are ions?
Atoms that have lost or gained electrons to become charged particles.
p.1
Trends in Element Properties
What are some properties you will investigate in relation to elements?
Electronegativity, first ionization energy, metallic and non-metallic character, and reactivity.
p.4
Subatomic Particles: Protons, Neutrons, and Electrons
How do protons and neutrons compare in terms of mass?
Protons and neutrons are almost identical in mass.
p.5
Subatomic Particles: Protons, Neutrons, and Electrons
How can you determine the number of neutrons in an atom?
By subtracting the atomic number (Z) from the mass number (A).
p.3
Subatomic Particles: Protons, Neutrons, and Electrons
What is the mass of a proton?
Approximately 1.673 x 10^-21 kg.
