1st Six Weeks Flashcards

Question

Potassium

Answer 1

Symbol: K Atomic Number: 19 Molar Mass: 39.10 Electron Configuration:

Answer 2

Symbol: Si Atomic Number: 14 Molar Mass: 28.09 Electron Configuration:

Answer 3

Symbol: Ag Atomic Number: 47 Molar Mass: 107.87 Electron Configuration:

Answer 4

Symbol: Na Atomic Number: 11 Molar Mass: 22.99 Electron Configuration:

Answer 5

Symbol: Sr Atomic Number: 38 Molar Mass: 87.62 Electron Configuration:

Answer 6

Symbol: S Atomic Number: 16 Molar Mass: 32.06 Electron Configuration:

Answer 7

Symbol: Sn Atomic Number: 50 Molar Mass: 118.71 Electron Configuration:

Answer 8

Symbol: Ti Atomic Number: 22 Molar Mass: 47.90 Electron Configuration:

Answer 9

Symbol: W Atomic Number: 74 Molar Mass: 183.85 Electron Configuration:

Answer 10

Symbol: Atomic Number: Molar Mass: Electron Configuration:

Answer 11

X axis: Independent variable | Y axis: Dependent variable

Answer 12

* Temperature change * Formation of bubbles * Color change * Formation of a precipitate

Answer 13

Homogenous mixture: a mixture which has uniform composition & properties throughout Heterogenous mixture: any mixture that is not uniform in composition

Answer 14

Mixtures can be separated by the process of evaporation, which is when a liquid is changed into a gas.

Answer 15

An extensive property is one that changes when the size of the sample changes. Ex: mass An intensive property is a physical one of a system that does not depend on the size or amount of material in the system. Ex: temperature

Answer 16

A physical property is any property that changes when the size of the sample changes. Ex: color, smell, melting point, etc. A chemical property is any of a material's properties that becomes evident during a chemical reaction. Ex: toxicity, flammability, reactivity, etc.

Answer 17

Precision: how close a measurement is to other values Accuracy: how close a measurement is to the actual value Uncertainty: that which you don't for certain; the last digit ("doubtful digit") in any quantitative measurement is uncertain

Answer 18

False: You always use the lowest number if there is one.

Answer 19

False: They are always significant.

Answer 20

Physical change: appearance changes but substance does not Ex: melting, breaking, cutting, etc. Chemical change: substance change Ex: produces bubbles, turns cloudy, change in smell or taste, etc.

Answer 21

Solid- molecules are closely packed, has a fixed position, rigid, cannot be squashed, has a fixed shape, cannot flow, and has a fixed volume (ex: computer) Liquid- molecules are closely packed (not as much as solids), not rigid, cannot be squashed, has no fixed shape, has a fixed volume, & can flow (ex: water) Gas- molecules are not closely packed (far apart), not rigid, can be squashed, has no fixed shape/volume, fill the whole space they're in (ex: helium) (4th state of matter)

Answer 22

``` Measure any physical quantity (ex: length) meter (m) -> length kilogram (kg) -> mass second (s) -> time mole (mol) -> amount of substance Kelvin (K) -> temperature cubic meter (m^3) -> volume ```

Answer 23

``` 1 mL = 1 cm^3 = 1 cc (volume) 1 L = 1,000 cm^3 1,000 L = 1 m^3 mm = milliliter cm = centimeter nano (n) = 10^-9 micro = 10^-6 milli (m) = 10^-3 centi (c) = 10^-2 kilo (k) = 10^3 mega (M) = 10^6 Angstrom = 10^-10 ```

Answer 24

Speed = distance/over (meters (m)/seconds (s))

Answer 25

He discovered atoms have electrons, which are much smaller

Answer 26

* Protons: Ernest Rutherford (1914) | * Neutrons: James Chadwick (1932)

Answer 27

1. Elements are composed of minute, discreet, and small particles called atoms. 2. Atoms of the same elements are different. 3. Compounds are composed of atoms of more than one element. In any compound, the combo of atoms is in fixed ratio of small whole numbers. 4. A chemical reaction involves the separation, combination, or rearrangement of atoms. It does not result in the destruction of the atoms, more the certain of other kinds of atoms. 1) All atoms of a given element are alike but the atoms of one element differ from the atoms of every other element. 2) All elements are made up of tiny, invisible, indestructible atoms. 3) Atoms are not created, destroyed, or converted into any other kinds of atoms during chemical reaction. They are simply rearranged into new compounds. 4) Compounds result from the chemical combination of a specific ratio of atoms or different elements.

Answer 28

When 2 elements combine in more than one proportion to form 2 or more compounds, the weights of one element that combine with a given weight of the other element are in the ratios of small whole numbers.

Answer 29

* The Cathode Ray Tube Experiment: J.J. Thompson and coworkers, 1897 * Dalton's Atomic Model: "All matter consists of tiny, indivisible particles. * Cathode rays must be made up of stuff that is negatively charged. * Particles that made up cathode rays are 1,000 times smaller than a hydrogen atom. * All different metals give off cathode rays. * Atoms have tiny, negatively charged particles inside them = Electrons. * Atoms are neutral. * There must be a positive charge in the atom to balance out the electrons.

Answer 30

* Hans Geiger, Ernest Marsden, and Ernest Rutherford (1911) * alpha particles: tiny, positively charged particles much smaller than an atom. * Hard dense nucleus w/positive charge

Answer 31

The Geiger–Marsden experiments (also called the Rutherford gold foil experiment) were a landmark series of experiments by which scientists discovered that every atom contains a nucleus where its positive charge and most of its mass is concentrated.

Answer 32

``` 1803- John Dalton •Atoms are made of even smaller particles. 1897- J.J. Thompson •Positively charged plate- anode •Negatively charged plate- cathode •Cathode rays come from cathode Electron discovered Ernest Rutherford •Discovered the atom's nucleus (99% of the atom's weight is concentrated here) •Discovered the proton •Atom's nuclear charge = the number of protons in nucleus = atomic number 1932- James Chadwick •Discovered neutrons •Helped invent atomic bomb ```