Chemistry chapter 4 Unit Test

How many electrons can a "d" sublevel hold?

10

How many neutrons does the isotope 125Te52? (first number is the superscript and second number is subscript)

73

The maximum number of electrons that can be found in any atom's second principal energy level is....

8

atomic mass symbol

A

the nucleus of a helium atom produced as the byproduct of a nuclear decay process

Alpha particle

the number of protons in the nucleus of the atom

Atomic Number (z)

electrons orbiting one or more atoms till the lowest available elergy levels before tilling higher levels

Aufbau principle

the number that defines the symmetrical shapes that are arranged around the nucleus and that electrons may be found in

Azimuthal quantum number

tritium is an isotope of hydrogen that has a mass number of three. What is its isotopic notation? (the first number is the superscript and the second number is the subscript) A. 1H1 C. 1H3 B. 3H1 D. 1H2

B

Be able to answer one of the three essays on the practice test.

Be able to draw a cathode ray tube

which of the following sets of quantum numbers is impossible?: A. 3,2,-3,+1/2 C. 1,0,0,-1/2 B. 2,1,0,-1/2 D. 4,1,1,+1/2

C

stream of electrons emitted from the cathode in the cathode-ray tube

Cathode Rays

who discovered the neutron?

Chadwick

What was the first model to include atoms of each element having different masses?

Dalton's atomic theory

concept that if waves can behave like particles, then particles can behave like waves

De broglie's hypothesis

Who was the first to refer to the smallest particles composing matter as atoms?

Democritus

known for their philosophical atomism

Democritus

who is known for discovering protons?

Ernest Rutherford

(true or false) An atom that gains three electrons will have a +3 charge.

False

(true or false) Neutrons contribute to an atom's mass and its charge.

False

(true or false) Scientific models are working representations of experimental facts that have been proven to be correct in all cases.

False

known for their gold foil experiment

Hans Geiger

the principle that it is impossible to know both the energy or momentum and the exact position of an electron at the same time

Heisenberg's Uncertainty principle

What describes how electrons fill a suborbital?

Hund's rule

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied

Hund's rule

Discovered Cathode Rays

J.J. Thomson

Discovered neutrons

James Chadwick

who did the first experimental atomic model?

John Dalton

states that every compound is formed of elements combined in mass ratios that are unique for that compound

Law of Definite Composition

What shows that any sample of water always contains 8 g of oxygen for every 1 g of hydrogen?

Law of definite composition

known for their "planetary" model of the atom

Niels Bohr

the rule that an orbital can hold only two electrons with opposite spin, resulting in a unique set of four quantum numbers for every electron

Pauli exclusion principle

known for magnetic resonance imaging

Raymond Damadian

(true or false) An electron can behave as either a wave or a particle.

True

(true or false) Dalton based his atomic model on both experimental evidence and logic

True

(true or false) Each atom can be identified by the number of protons in the nucleus

True

(true or false) The first quantum number identifies the principal energy level of an electron.

True

(true or false) The general region of space where an electron is most probably found is known as an orbital.

True

standard unit that is used for indicated mass on an atomic or molecular scale

Unified atomic mass unit

What was Thomson's cathode rays?

Valence electrons

the electrons in the outermost energy level that are important in bonding are called __________ _____________.

Valence electrons

Discovered X-rays

Wilhelm Roentgen

What is a negatively charged ion called?

an anion

a negatively charged ion

anion

smallest particle that makes up an element

atom

The s,p,d, and f sublevels are identified by ______ quantum numbers.

azimuthal (l)

be able to write electron and orbital notations

be able to write the isotopic notation

a positively charged ion

cation

the complete visual spectrum with no frequency gaps, emitted only by an ideal luminous object

continuous spectrum

Which has the least mass- an electron, a proton, or a neutron?

electron

what is an atomic particle with a negative charge?

electron

the description of electrons as moving independently

electron configuration

a way of representing atoms or molecules by showing electrons

electron dot notation

the number that describes the two possible "spin" states of a pair of electrons in an orbital

electron-spin quantum number

an atom's lowest energy state

ground state

One of two or more atoms of the same ele- ment with the same number of protons but with different numbers of neutrons.

isotope

A naming convention used to distinguish between different isotopes of elements.

isotopic notation

a spectrum showing only certain colors or wavelengths of light

line spectrum

MRI machines make images through changing ____ in an atom.

magnetic fields

the number that defines the spatial orientation of the orbitals within a sublevel

magnetic quantum number

the neutral part of an atom's nucleus

neutron

the dense, central part of the atom

nucleus

3-D region of space around the nucleus in which as many as2 electrons are likely to be found; they also make up sublevels

orbital

another way of writing the electron configuration

orbital notation

packet of electromagnetic energy modeled as a particle that transmits electromagnetic force int he standard model of matter

photon

if an atom loses an electron, the atom will have a _________ charge.

positive

region around the nucleus containing a specified group of electrons in sublevels and orbitals

principal energy level

Niels Bohr, in his model of the atom, proposed the concept of ________ that were envisioned as a set of concentric circular tracks on which ___________ orbited.

principal energy levels/ electrons

the number indicating the main/principal energy level in which an electron is found

principal quantum number (n)

atomic structure with a positive charge

proton

The mass number = the number of _________ and the number of __________.

protons/neutrons

Two different isotopes of a single element would have the same number of ____ but a different number of ________.

protons/neutrons

having to do with quantities in which there are only separate, discrete values allowed

quantize

because energy levels are ___________, energy emissions come in certain quantities.

quantized

describes the location of an electron in an atom

quantum number

The type of sublevel found in all principal energy levels is the ____ sublevel.

s

the portion of a principal energy level made up of one or more orbitals

sublevels- spdf

What describes how electrons fill orbitals?

the Aufbau principle

What helped explain line spectra?

the Bohr model of the atom

What states that it is impossible to know both the energy and the exact position of an electron at the same time?

the Heisenberg uncertainty principle

What states that no two electrons in an atom can have the same set of four quantum numbers?

the Pauli exclusion principle

what subatomic particle was discovered through experimentation with cathode rays?

the electron

electron associated with an atom

valence electron