Science Lesson 1: Properties of Matter

<p>Plum Pudding Model (C)</p> Signup and view all the answers

<p>It provided evidence for the existence of negatively charged particles. (D)</p> Signup and view all the answers

<p>Dalton believed that atoms were indivisible, while Rutherford discovered subatomic particles. (A)</p> Signup and view all the answers

<p>It allowed the study of the behavior of negatively charged particles. (D)</p> Signup and view all the answers

<p>A shorthand representation of a chemical element consisting of one or two letters derived from the element's name. (A)</p> Signup and view all the answers

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

<p>The number of neutrons in their nuclei. (A)</p> Signup and view all the answers

<p>Number of isotopes present. (D)</p> Signup and view all the answers

<p>By subtracting the atomic number from the mass number. (A)</p> Signup and view all the answers

<p>It determines the element's chemical properties. (D)</p> Signup and view all the answers

<p>Half-life (D)</p> Signup and view all the answers

<p>The arrangement of electrons in the electron shells around the nucleus. (B)</p> Signup and view all the answers

<p>Nuclear reactions. (D)</p> Signup and view all the answers

<p>Quantum Mechanical Model (B)</p> Signup and view all the answers

<p>The shape of the sublevel (B)</p> Signup and view all the answers

<p>The larger the value of <em>n</em>, the further it is away from the nucleus, and thus the higher the energy of an electron. (A)</p> Signup and view all the answers

<p>The bigger the cloud, the more electrons. (D)</p> Signup and view all the answers

<p>A group of orbitals with the same shape. (D)</p> Signup and view all the answers

<p>To describe the orientation of an orbital in space. (A)</p> Signup and view all the answers

<p>To describe the distribution of electrons in each energy level. (C)</p> Signup and view all the answers

<p>Describing the mass of an electron. (D)</p> Signup and view all the answers

<p>The energy level and distance from the nucleus (B)</p> Signup and view all the answers

<p>10 (D)</p> Signup and view all the answers

<p>Orbitals are filled with one electron each before any orbital is doubly occupied. (B)</p> Signup and view all the answers

<p>An atomic orbital describes the shape of an electron's wave pattern, while an energy level describes the electron's energy. (C)</p> Signup and view all the answers

<p>The direction of an electron's spin. (A)</p> Signup and view all the answers

<p>To visually depict the distribution of electrons in an atom's orbitals. (C)</p> Signup and view all the answers

<p>The atomic number determines the number of protons and electrons, which is then used to fill the energy levels (n) in the electron configuration. (D)</p> Signup and view all the answers

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

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

<p>A characteristic that can be observed or measured without changing the chemical composition of a substance. (D)</p> Signup and view all the answers

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

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

<p>Mass measures the amount of matter, weight measures the force of gravity on the matter. (B)</p> Signup and view all the answers

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

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

<p>It moves to a higher energy level. (D)</p> Signup and view all the answers

<p>The farther the distance, the higher the energy. (B)</p> Signup and view all the answers

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

<p>In a neutral atom, the atomic number is equal to the number of electrons. (D)</p> Signup and view all the answers

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

<p>It has lost or gained electrons. (A)</p> Signup and view all the answers

<p>The outermost energy level. (D)</p> Signup and view all the answers

<p>It replaced the idea of fixed orbits for electrons with probabilistic regions. (C)</p> Signup and view all the answers

Particles smaller than an atom that make up matter.

An English physicist who proposed the atomic theory in 1808.

Theory that matter is composed of atoms, indivisible and unique to each element.

A vacuum tube that generates streams of electrons used in experiments.

Physicist who discovered the electron using the cathode ray tube in 1897.

A model where electrons are embedded in a positively charged sphere.

Dalton's model of the atom, describing atoms as solid, indivisible spheres.

A tiny, negatively charged particle discovered by Thomson.

Smallest building blocks of protons and neutrons.

Basic units made of electrons, protons, and neutrons.

Properties that depend on the amount of substance present.

Observable characteristics that do not change chemical composition.

Ability to return to original shape after stretching or compressing.

Ability of an object to shatter easily.

Temperature at which a substance transitions from liquid to gas.

Temperature at which a substance transitions from solid to liquid.

Regions around the nucleus where electrons can reside, each with a specific distance and energy.

The transition of electrons from lower to higher energy levels through absorption or emission of energy.

A modern atomic model that depicts probabilistic regions rather than fixed orbits for electron locations.

The atomic number (Z) represents the number of protons in the nucleus of an atom, determining the element.

Positively charged ions formed when an atom loses one or more electrons.

Negatively charged ions formed when an atom gains one or more electrons.

The outermost energy level of an atom, containing the valence electrons that participate in chemical bonding.

Processes by which electrons gain energy (absorption) or lose energy (emission) to move between energy levels.

Electrons can spin in two directions: +½ (clockwise) or -½ (counterclockwise).

Regions of space where there is a high probability of finding electrons.

Different orbitals can hold different maximum numbers of electrons: s=2, p=6, d=10, f=14.

Indicates the energy level and size of an electron's orbital.

Visual representations showing electron distribution in orbitals.

Electrons fill empty orbitals first before pairing up in one.

The notation that shows the distribution of electrons among orbitals.

Energy changes occur when electrons shift between different wave patterns.

Atoms of the same element with different numbers of neutrons.

The number of protons in an atom's nucleus, defining the element.

A one or two-letter abbreviation for a chemical element.

The difference between the mass number and the atomic number.

The total number of protons and neutrons in an atom's nucleus.

The average mass of an atom of an element, accounting for all particles.

The time required for half of a sample of an isotope to decay.

The process by which unstable isotopes lose energy by emitting radiation.

The center of the atom, containing protons and neutrons.

Indicates the shape of orbitals within an energy level, ranging from 0 to (n - 1).

Groups of orbitals within an energy level sharing the same shape.

Describes the orientation of an orbital in three-dimensional space.

Indicates the spin state of an electron within an orbital.