Exam Flashcards
Electromagnetic radiation is a kind of
Energy
that behaves like a(n)
Wave
is one type of electromagnetic radiation. Other examples include X rays, radio waves, and microwaves. All waves can be characterized by their wavelength, amplitude, frequency,
Speed
The shortest distance between equivalent points on a continuous wave is called a(n)
wavelength
The height of a wave from the origin to a crest or from the origin to a trough is the
amplitude
is the number of waves that pass a given point in one second
Frequency
Wavelength is measured in
Meters
That has the symbol?
M
We measure frequency in
Hertz
That has the symbol
Hz
A(n) is the minimum amount of energy that can be lost or gained by an atom.
quantum
The is the phenomenon in which electrons are emitted from a metal’s surface when light of a certain frequency shines on it.
photoelectric effect
When an atom emits light, photons having certain specific energies are being emitted.
True
A flame test cannot be used to identify the presence of certain elements in a compound.
False
The fact that only certain colors appear in an element’s atomic emission spectrum indicates that only certain frequencies of light are emitted
True
Atomic emission spectra can be explained by the particle model of light.
False
The neon atoms in a neon sign emit their characteristic color of light as they release energy
True
Like the visible spectrum, an atomic emission spectrum is a continuous range of colors.
False
When an atom emits light, photons having certain specific energies are being emitted.
True
Each element does not have a unique atomic emission spectrum.
False
There are three main classifications of elements.
True
There are three main classifications of elements.
True
Group 7A elements are highly reactive nonmetals known as noble gases.
False
Group 4A elements are the alkaline earth metals.
False
Alkaline earth metals do not react with oxygen.
False
Alkali and alkaline earth metals are not reactive.
False
The metal lithium has a diagonal relationship with the metal aluminum.
False
An alloy is a compound of two or more metals.
True
Alkali metals are shiny gray solids soft enough to be cut by a knife.
True
The order of reactivity of the alkaline earth metals, from least to most reactive, is beryllium, magnesium, calcium, strontium, and barium.
True
Sodium and potassium are the most abundant alkali metals.
True
Sodium and potassium are the most abundant alkali metals.
True
Barium chloride can be used as a substitute for sodium chloride.
False
Alkaline earth metals form ions with a 2+ charge.
True
The ending -ide is used to designate an anion.
True
The ending -ide is used to designate an anion.
True
Elements in group 1A lose their one valence electron, forming an ion with a 1- charge
False
The electron structure of a zinc ion ( Z n 2 \+ Zn 2+ ) is an example of a pseudo-noble gas formation.
True
A positively charged ion is called an anion.
False
The lowest allowable energy state of an atom is called its
Ground states
Bohr’s model of the atom predicted the
Frequencies
According to Bohr’s atomic model, the smaller an electron’s orbit, the
Lower
According to Bohr’s atomic model, the larger an electron’s orbit, the
Higher
Bohr proposed that when energy is added to a hydrogen atom, its
Electron
According to Bohr’s atomic model, the hydrogen atom emits a photon corresponding to the difference between the
Energy levels
Bohr’s atomic model failed to explain the blank of elements other than hydrogen.
Atomic emission spectrum
Atomic orbitals blank have an exactly defined size
Do not
Each orbital may contain at most electrons.
Two
The maximum number of blank related to each principal energy level equals
Electron
Principal energy level 2 consists of
2s and 2p
Strontium - period:
Valence electron:
Block:
Period: 5
Block: s
Valence electron: 2
Potassium
Period: 6
Block: d
Valence electron: 2
Osmium -
Period: 6
Block:d
Valence electron: 2
According to Planck’s theory, for a given frequency, ν ν , matter can emit or absorb energy only in
whole-number multiples of hν
Which equation would you use to calculate the energy of a photon?
E photon=hν E photon
=hν
The modern model of the atom that treats electrons as waves
quantum mechanical model of the atom
Originally applied to the hydrogen atom, it led to the quantum mechanical model of the atom
Schrödinger wave equation
States that it is impossible to know both the velocity and the position of a particle at the same time
Heisenberg uncertainty principle
A three-dimensional region around the nucleus representing the probability of finding an electron
atomic orbital
The arrangement of electrons in an atom is called the atom’s
electron configuration
Electrons in an atom tend to assume the arrangement that gives the atom the
Lowest
This arrangement of electrons is the most arrangement and is called the atom’s ground-state.
Stable and electron configuration
states that each electron occupies the lowest energy orbital available.
Aufbau principle
The Pauli exclusion is
principle
states that a maximum of two electrons may occupy a single atomic orbital, but only if the electrons have opposite
spins
states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins occupy the same orbitals.
Hund’s rule
Give the ground state electron configurations for the following elements. Use the following format:principle quantum number, sublevel, number of valence electrons, repeat. You do not have to use the ^ for the exponent
Carbon: 1s^2 2s^2 2p^2 1s^2 2s^2 2p^2
Chromium
1s^ 2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^4
The s-block contains groups
1A and 2A
How many d-block elements are there? (number)
40
There are blank f-block elements. (number)
28
The table below was developed by John Newlands and is based on a relationship called the law of
octaves
According to this law, the properties of the elements repeated every
Eight element
Thus, for example, element two and element
Nine
have similar properties. The law of octaves did not work for all the known elements and was not generally
Accepted
The first periodic table is mostly credited to
Dmitri Mendeleev
In his table, the elements were arranged according to increasing
Atomic mass
