Untitled Flashcards Set

Quantum particles They have no mass, and travel at or near the speed of light.
Wave-particle duality Quantum particles act as both a particle and a wave at the same time.
Bohr's model Requires an atom to absorb a specific, discrete packet size of energy acting as a particle, and emit the same energy, which is perceived as color (wave).
Formula for speed of light c = λ f, where c is the speed of light, λ is wavelength, and f is frequency.
Planck's equation E = h f, where E is energy, f is frequency, and h is Planck's constant (approximately 6.64E-34 J/Hz).
Electromagnetic spectrum trend Moving from left to right (R O Y G B I V), wavelength (λ) decreases, frequency (f) increases, and energy (E) increases.
Electron transitions Colored lines in spectra represent electrons falling from a higher to a lower energy level, emitting energy.
Energy packet size Refers to energy sizes that the atom did not absorb, which pass through without interacting.
Uncertainty principle You cannot know the exact speed and exact location/path of a quantum particle at the same time.
Orbital The 3-D region of space outside the nucleus where there is the highest probability of finding an electron.
Valence electrons Electrons in the outermost energy level of an atom.
Energy level The distance of valence electrons from the nucleus and the number of valence electrons.
Ionic compound A compound formed from the transfer of electrons between atoms, resulting in charged ions.
Covalent bond A bond formed through the sharing of electrons between atoms.
Metallic bond A bond between positively charged metal ions and a freely moving 'sea of electrons', occurring in two or more metals.
Location of nonmetals Nonmetals are found on the right side of the periodic table.
Emission spectra The specific wavelengths of light emitted by electrons transitioning between energy levels in an atom.
Bohr's explanation of atomic interactions Bohr proposed that atoms absorb and emit energy in discrete amounts, leading to quantized energy levels.
De Broglie's theory Suggested that particles, like electrons, exhibit both particle and wave-like properties, leading to the concept of matter waves.
Valence electrons (revised) Electrons in the outermost energy level of an atom that participate in chemical bonding.
Shared valence electrons in nonmetals Nonmetals can share valence electrons in covalent bonds, resulting in molecules.
Properties of nonmetals Nonmetals tend to have lower melting and boiling points, are poor conductors of heat and electricity, and are typically brittle.
Properties of metals Metals are good conductors of heat and electricity, malleable, ductile, and generally have high melting and boiling points.
Chemical compound names Compounds formed from metals and nonmetals are generally ionic compounds, while those formed from nonmetals are covalent compounds.
Resulting particle names from ionic bonding Ionic compounds result in charged particles called ions, specifically cations (positively charged) and anions (negatively charged).
Condition for larger particle size In ionic compounds, lower charge (cf) usually correlates with larger ionic radius, while higher charges attract ions more closely, resulting in smaller sizes.
Example of a covalent bond Water (H2O) is a molecule formed by covalent bonds between hydrogen and oxygen sharing valence electrons.
Comparative size of metals vs nonmetals In general, metal ions are smaller than their neutral atoms, while nonmetal ions are larger than their neutral atoms due to the gain or loss of electrons.
What happens to wavelength in the electromagnetic spectrum from red to violet? Wavelength decreases as you move from red (longest wavelength) to violet (shortest wavelength) in the electromagnetic spectrum.
What happens to frequency in the electromagnetic spectrum from red to violet? Frequency increases as you move from red to violet in the electromagnetic spectrum.
What happens to energy in the electromagnetic spectrum from red to violet? Energy increases as you move from red to violet in the electromagnetic spectrum.
Relationship between wavelength and frequency in the electromagnetic spectrum Wavelength and frequency are inversely related; as one increases, the other decreases.
What is the significance of the ROYGBIV sequence in the electromagnetic spectrum? ROYGBIV represents the visible spectrum, with red being the lowest energy and frequency, and violet being the highest.