Unit 1 Intro & Measurement Flashcards by Bella Fernandez

Describe the solid state of matter

-definite volume
-maintains shape regardless of container
-particles are close together and in a regular pattern
-high density

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Describe the liquid state of matter

-definite volume
-takes shape of its container
-particles are close together and move past each other -difficult to compress

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Describe the gas state of matter

-no definite shape
-assumes shape of container
-no definite volume
-particles are far apart and move around randomly

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Describe the plasma state of matter

-highly charged particles
-high kinetic energy
-no fixed shape or volume
-less dense than solids or liquids
-ions roam freely

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What is a mixture?

-composed of more than 1 component
-varying composition
-any combo of solid, liquid, or gas
-can be separated into its components by physical process

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Examples of mixtures

-sugar dissolved in water
-salt water
-air (mix of gases)
-solutions, colloids, suspensions

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What are the 2 types of mixtures & describe them

-heterogeneous mixture = visually distinguishable components (salt & pepper, oil & water)

-homogeneous mixture = appear uniform throughout, all solutions are homogenous not all homogenous mixtures are solutions (milk: uniform appearance, but still has fat particles floating around)

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What is matter?

anything that has mass / takes up volume

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What 2 categories can matter be divided into based on its PHYSICAL changes ?

pure substances & mixtures

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What is a pure substance?

-composed of only a single component (atom or molecule)
-has a consistent composition
-cannot be broken down into other pure substances by a physical change
-either an element or a compound

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How is a pure substance different from a mixture?

-mixtures are composed of more than one component
-mixtures have varying composition
-mixtures can be separated into their components by physical process

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What is an element?

a pure substance that cannot be broken down by a chemical change

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What is a compound?

a pure substance formed by chemically joining two or more elements chemical combo of 2 or more elements (salt = NaCl, water H2O)

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What two things can be separated by CHEMICAL means?

compounds & molecules

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What is an atom?

the building blocks of all matter

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What is a molecule

-a group of atoms bonded together
-the smallest unit of a chemical compound that can take part in a chemical reaction
-elements contain molecules, compounds are molecules of that compound

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What are diatomic molecules?

molecules that contain 2 atoms that are chemically bonded

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What are the 7 naturally occurring diatomic molecules?

-Hydrogen (gas)
-Nitrogen (gas)
-Fluorine (gas)
-Oxygen (gas)
-Iodine (solid)
-Chlorine (gas)
-Bromine (liquid)

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What are physical properties?

things that can be measured without changing the composition of the sample under study

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Examples of physical properties

-mass
-color
-volume
-density
-solubility
-odor
-melting point / boiling point

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What are chemical properties

chemical reactions / changes

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Examples of chemical properties

-flammability
-toxicity
-heat of combustion
-pH value
-rate of radioactive decay
-chemical stability

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What are the signs that a chemical change occurs?

-color change
-formation of precipitate
-formation of gas
-odor change
-temperature change
-production of light
-volume change
-change in taste or smell
-formation of bubbles

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“mega” prefix meaning

10^6

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"kilo" prefix meaning

10^3

"deci" prefix meaning

10^-1

"centi" prefix meaning

10^-2

"milli" prefix meaning

10^-3

"micro" prefix meaning

10^-6

"nano" prefix meaning

10^-9

What are the building block elements of the human body (96%)

-oxygen -carbon -hydrogen -nitrogen

What are the 3 subatomic particles that atoms are composed of?

-protons -neutrons -electrons

Describe the nucleus

-location of protons and neutrons -dense core of the atom -location of most of the atom's mass

Describe the electron cloud

-location of electrons -comprises most of the atom's volume -mostly empty space

Atomic number is equal to what?

the number of protons in the nucleus

What are isotopes?

atoms of the same element that have different #s of neutrons *same atomic number, different mass number*

What are principal energy levels / shells (n)?

the region around the nucleus that is occupied by electrons with particular energy

Which electrons are closer to the nucleus?

electrons in the lower numbered shells

Which electrons are further from the nucleus?

electrons in higher numbered shells

What are the subshells labeled as & how many orbitals do they each have?

- s = 1 orbital - p = 3 orbitals - d = 5 orbitals - f = 7 orbitals

How many electrons can each orbital hold?

What are orbitals?

region of space where the probability of finding an electron is high

List the properties of metals

-located on the left side & middle of the periodic table -good conductors of heat and electricity -malleable (thin sheets) -ductile (thin vials) -shiny solids at room temperature (except mercury (Hg) which is a liquid)

List the properties of nonmetals

-located on the right side of the periodic table -have a dull appearance -usually poor conductors of heat & electricity -can be solids, liquids or gases at room temp

List the properties of metalloids/semi-metals

-located on the solid line that starts at boron (B) and angles down towards astatine (At) -have properties intermediate between metals and nonmetals -**only 7 metals are metalloids: boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), & astatine (At)

What is specific gravity?

-a quantity that compares the density of a substance with the density of water at the same temperature

What is the density of water?

1g/mL

How many elements are there?

117

Major minerals:

elements that are needed (at least 100mg daily) -magnesium & sulfur

Mass number =

number of protons + number of neutrons

#of neutrons =

atomic mass - atomic number

hydrogen

helium (noble gas)

lithium (alkali metal)

beryllium (alkaline earth metal)

boron (metalloid)

carbon (non-metal)

nitrogen (non-metal)

oxygen (non-metal)

fluorine (halogen)

neon (noble gas)

sodium (alkali metal)

magnesium (alkaline earth metal)

aluminium (metal)

silicon (metalloid)

phosphorous (non-metal)

sulfur (non-metal)

chlorine (halogen)

argon (noble gas)

potassium (alkali metal)

calcium (alkaline earth metal)

scandium (transitional metal)

titanium (transitional metal)

manganese (transitional metal)

iron (transitional metal)

cobalt (transitional metal)

nickel (transitional metal)

copper (transitional metal)

germanium (metalloid)

arsenic (metalloid)

bromine (halogen)

krypton (noble gas)

silver (transitional metal)

antimony (metalloid)

tellurium (metalloid)

iodine (halogen)

gold (transitional metal)

mercury (transitional metal)

lead (metal)

What is atomic weight?

the weighted average of all the masses of the naturally occurring isotopes of a particular element (located below the chemical symbol)

What is the unit for atomic weight?

amu (atomic mass units)

how do you calculate amu?

(fraction (%) of 1 isotope x mass of isotope 1) + (fraction of isotope 2 x mass of isotope 2)...

what is natural abundance?

the amount the particular isotope/element is naturally occurring

isotopic abundance needs to be:

in decimal form

halogens

-only exist as two atoms together (diatomic) -very reactive

noble gases

-very stable -rarely reactive with other elements

alkali metals & alkaline earth metals

-soft* shiny metals -good conductors of heat and electricity

what is the formula for calculating how many electrons each shell can hold ?

2n^2

What are valence electrons?

Valence shell = the outermost shell (highest value of n), the electrons in that shell are valence electrons

What is the Lewis structure?

electron-dot structure , it represents the valence electrons of a particular element

Why does atomic size increase as we go down a group on the periodic table?

Because the number of shells increases

Why does atomic size decrease as we go left to right on the periodic table?

the number of electrons is increasing, therefore attracting more energy and shrinking its size

What is ionization energy?

the energy needed to remove an electron from a neutral atom

Why does ionization energy decrease as we go down the periodic table?

valence electrons get farther away from the positively charged nucleus

Unit 1 Intro & Measurement Flashcards

(104 cards)