Exam

Proton

positively charged particle

Elements within the same group or family have similar ______

properties

Which subatomic particles are found in the atoms nucleus?

protons and neutrons

A cation always has more ____

protons than electrons

Mass is a measure of the ____ of matter

quantity

Energy

the ability to do work

Heterogenous mixture

A mixture that is not uniform throughout

homogenous mixture

A mixture with a uniform composition throughout

The isotope of 15N has a net ruin number of _______

8

Which correctly describes physical properties A. Characteristics that can be observed or measured without changing the composition of a substance B. The state of a sample, such as solid, liquid, or gas C. Properties that can be measured when burning a substance in the air D. The composition of a compound

A

Select which describe volume A. The volume of a cube is equal to length x width x height B. Is a 3D quantity C. Is a type of qualitative physical property D. Is the amount of space a substance occupies E. Vol of a sphere = 4/3 x pi x r

A, B, and D

Which are True A. Some elements have been synthesized by scientists B. Elements are building blocks of matter C. All elements are stable and do not break down over time D. Some elements are isolated from natural sources on earth

A, B, and D

Which are true A. Metals conduct electricity B. Metals conduct heat C. Metals are all silver in color D. Metals are shiny

A, B, and D

Which are examples of physical changes A. Mixture is separated into its components B. Sample is heated and it melts C. Electricity is used to change water into H and O2 gases D. A fuel is burned in air to form co2 and h20 E. Water evaporates slowly over time

A, B, and E

Which are true of a chemical formula A. Uses subscript numbers to show the relative proportions of the elements in the compound B. A subscript present in a chemical formula applies to all elements preceding it in the formula C. A mixture is represented with a chemical formula D. Describes the composition of a compound using the symbols for the elements that make up the compound E. A chemical formula does that does not contain subscript numbers consists of a one-to-one ratio of the events that are present

A, D, and E

quantitative observation

Based on number

qualitative observation

Based on quality of matter

Physical Changes in Matter

Change in form or appearance

Using an oil drop apparatus, Robert Millikan determined that the ______ of the _______ was 1.6022 x 10^-19 coulombs

Charge, electron

When nonmetals form ions they _____

Form anions and gain electrons

When nonmetals form ions they ______

Form ions and gain electrons

gas symbol

G

To achieve the stability of a noble gas, elements in group VIIA _____ an electron to be like the closest noble gas

Gain

When nonmetals form ions they ________

Gain electrons form anions

Process of naming acids that do not contain polyatomic ions A. Write suffix -ic B. Write word acid C. Write stem name of the non hydrogen element in the acid D. Write prefix hydro

D, C, A, B

The law of definite proportions predicts that a sample of pure iron(II) oxide (FeO) mined in northern Canada would have the same ______ as a sample of pure iron (II) oxide mined in the western United States

Iron to oxygen ratio

Celsius to Kelvin

K=C+273.15

Sodium symbol

Na

Iodine is a _______

Nonmetal

Metalloids have properties similar to ____

Nonmetals and metals

Which of the following elements will form 2- ions? A. Chlorine B. Oxygen C. Bromine D. Sulfur N. Nitrogen

Oxygen and Sulfur

The mass number of an isotope can be described as the sum of the number of ____ and ____ in that isotope

Protons and neutrons

Rutherfords gold foil experiment provided evidence for _______

Dense, positively charged mass in the center of an atom

T/F : the relative atomic mass shown on the periodic table is the sun of the masses of all isotopes of an element

Fakse

T/F : the relative atomic mass shown on the periodic table is the sum of the masses of all isotopes of an element

False

In general, metals ___ electrons to form ____ when they form ions, giving them the same electron count as the nearest noble gas

Lose, cations

The total number of protons and neutrons in an isotope gives the isotopes _____

Mass number

A ___ consists of two or more ____ and may vary in composition

Mixture, pure substances

An example of matter is correctly described by which? A. Energy is an example of matter bc it Uc u pies space and has mass B. A textbook is an example of matter bc it occupies space and has mass C. Heat is an example of matter because it occupies space and mass D. Sunlight is an example of matter because of its capacity to transfer heat

B

Which are monatomic anions? A. CN- B. O2- C. Cl- D. O2^-2

B and C

Which correctly describes the isotopes of an element? A. All atoms in a natural sample of the element contain the same number of neutrons B. All atoms in a natural sample of an element contain the same number of protons C. All atlms in a natural sample of an element contain the same number of electrons

B and C

which equations represent chemical formulas A. H2O(I) -> H2O(s) B. 2H2(g) + O2(g) -> 2H2O(g) C. C(s) + O2(g) -> CO2(g) D. CO2(s) -> CO2(g)

B and C

Which are general properties of the noble gases A. Reactive B. Stable C. Easily form ions D. Inert

B and D

Which describes density A. When comparing equal masses of two different substances, the substance with the greater volume has the greater density B. The density of a substance changes with changing temperature C. The density of a substance depends on the amount of substance that is present D. The density of an object is the ratio of its mass to its volume

B and D

Which are anions A. 15 p, 15 e, 16 n B. 16 p, 18 e, 16 n C. 23 p, 23 e, 27 n D. 17 p, 18 e, 18 n

B and D More electrons than protons

An atom in which the number of electrons is different from the number of protons is an ____

Ion

law

The behavior of matter that is so consistent that it appears to have universal validity

absolute zero

The lowest possible temperature in the universe

Put the following in order of increasing mass 1 ug 1 mg 1 Gg 1 Mg 1 dg

Ug, mg, dg, Mg, Gg

Silicon is a ______

metalloid

A sample of matter that consists of a combination of two or more pure substances is called a _______. The combination may vary in its __________.

mixture & composition

A neutron is a subatomic particle that is found in the ______ of an atom

nucleus

A ____ is the smallest unit of an element that has the chemical properties of that element. Two or more of these units can be bound together in a discrete arrangement form a _______

atom, molecule

Polyatomic ions are ions that contain two or more _____

atoms

In an atom that is neutral, the number of protons is _______ the number of electrons

equal to

liquid to gas

evaporation

kinetic energy

energy of motion

The law of conservation of mass states that in a chemical reaction _____

mass will remain constant when reactants turn into products

Magnesium is a _____

metal

The inner transition elements are shown below the main blocks of the periodic table, however, these elements belong ______

after lanthanum and actinium

gas to liquid

condensation

gas to solid

deposition

The density of solid gold at room temp is 19.3 g/mL. Given a 45 mg sample of gold, what is the volume in mL

2.3 x 10 ^-3 mL 45 mg = .045 g .045 g / 19.3 g per mL = .0023

The number of protons in an atom of the element calcium is ____

20

Solve for the mass of a 3.5 x 10^5 cg sample in units of kg

3.5 kg

Potassium has an isotope with 20 neutrons. What is the mass number?

39

Which describes an atomic nucleus A. The nucleus is composed of protons and neutrons B. The size is small compared to the overall size of the atom C. The nucleus takes up the most space in an atom

A and B

Which are homogenous mixtures A. A well mixed sample of sugar water B. Pure water containing no additional components C. A red sports drinks with sugar, salt, and food coloring D. A jar of chunky salsa

A and C

Which of the following statements describes the nuclear model of the atom? A. Most of an atoms mass is found in the nucleus B. Electrons are found throughout the entire volume of the atom, including the nucleus C. An atom has a uniform density throughout the entire atom D. An atom is mostly empty space

A and D

Which choices describes an ion A. 25 p, 20 e, 29 n B. 35 p, 35 e, 44 n C. 47 p, 47 e, 58 n D. 8 p, 9 e, 8 n

A and D Ions have diff numbers of electrons than protons

Select all that correctly state a metric conversion A. 1 kg / 10^3 g B. 1 Mg/10^-3 g C. 10^-6 ug / 1 g D. 10^-2 cg / 1 g E. 1 ng / 10^-9 g

A and E

Scientific Method

An approach to asking questions and seeking answers that employs a variety of tools, techniques, and strategies

combinatorial chemistry

A series of related chemical compounds is systematically prepared and tested for effectiveness

element symbol

A short hand version of an element's longer name

Aqueous

dissolved in water

In order to determine the relative atomic mass of an element, one should ______ A. Use the mass of the most abundant isotope as the average B. Calculate the straight average of the masses of all isotopes C. Take a weighted average of the masses of all isotopes using their abundance

C

Which correctly display the relationship between 1 milligram and 1 gram A. 1Mg/10^-3g B. 10^3 g / 1 mg C. 10^-3 g / 1 mg D. 1 g/10^3 mg E. 1 g/10^-3 mg

C and D

Which describe chemical properties A. Can be observed directly in all cases B. A characteristic that can be measured or observed without changing the composition of the substance C. Can be defined by what chemical changes it can undergo D. Can be defined by the composition of the substance

C and D

Which represent chemical properties A. Melting point B. Density C. Reactivity with water D. Flammability E. Solubility in water

C and D

Hypothesis

A tentative explanation for the properties or behavior of matter that accounts for a set of observations

Solution

A type of homogeneous mixture that is typically composed of a substance in lesser amount dissolved in a substance in greater amount

Dalton's Atomic Theory, but not our modern atomic theory, atoms are described as ______

small and indivisible

solid to gas

sublimation

Steps to naming the compound Co(CH3CO2)3

1. Identify the cation as cobalt and the anion as acetate 2. Identify the charge of acetate as -1 3. Write the name if the cation cobalt and determine its charge as 3+ 4. Write the Roman number III 5. Write the name of the anion acetate

solve for the volume of a 1.5 x 10^6 cm^3 object in units of liters

1.5 x 10^3 L 1 cm^3 = .001 L 1.5 x 10^6 cm^3 = 1.5 x 10^6 = .001 L = 1500 L 1500 L = 1.5 x 10^3 L

Solve for the mass of 85.4 kg in units of pounds

1.88 x 10^2 85.4 kg = 188.27160 lb

Selenium symbol

Se

Silicon symbol

Si

liquid to solid

freezing

Celsius to Fahrenheit

(C x 1.8) + 32

Fahrenheit to Celsius

(F-32)/1.8

aqueous symbol

(aq)

The mass number and atomic number for iodine-128 are ______ respectively

128 and 53

Neutron number for 25Mg is

13 Atomic # + neutron # = mass #

List the temps in order of increasing temp 48° F 48° K 48° C

48°K, 48° F, 48° C

Which are True A. The elements in each column of the periodic table share similar properties B. Each column in the periodic table is called a group or family of elements C. The periodic table is used by chemists to classify mixtures D. The elements in each of the periodic table share similar properties

A and B

Which are true A. Solids, liquids, and gases are examples of physical states of matter B. The physical state of a substance depends on the identity of the substance and the external conditions applied C. The arrangement of particles is independent of the physical state of the substance D. At room temperature, the physical state of any substance is a liquid

A and B

Mixture

A physical combination of two or more elements or compounds

Which about density are true A. A substance with a large mass/vol is less dense than a substance with a small mass / vol B. A solid object with a greater density than a liquid substance will sink in the liquid C. When mercury (d=13.6 g/mL) and water (d=1 g/mL) are mixed, the mercury floats in water D. If mass and density of a pure substance are known, the volume can be calculated for the substance E. In general gases have very low densities because gas particles spread out and occupy large volumes

B, D, and E

Which express units of volume A. mL^3 B. yd^2 C. qt D. cm^3 E. L

C, D, and E

What is the formula for cobalt (II) hydroxide

Co(OH)2

Common properties of elects on the periodic table are emphasized by the arrangement of elements within ______

Columns and rows

JJ Thomson's cathode ray experiment was important for its discovery of _____

Electrons

Which of the following subatomic particles are NOT found in the nucleus of the atom? Protons Electrons Neutrons

Electrons

potential energy

Energy possessed by an object because of its position or state

8 grams of methane gas is burned with 32 g of oxygen gas inside a strong, sealed vessel that prevents the escape of the heat, water and carbon dioxide produced. The mass of the flash and it's contents before the reaction will be _____ the mass of the flask and it's contents after the reaction

Equal to

Theory

Explains why observations, hypotheses, or laws apply under many different circumstances

The alkaline earth metals are found in which group?

Group IIA

Solid

Has a fix shape, has its own volume, has particles that are fixed in place

liquid symbol

L

The relative atomic mass of lithium is 6.941 amu. There are two isotopes of lithium, Li-6 and Li-7. Which is more abundant?

LI 7

Sulfur symbol

S

solid symbol

S

Tin symbol

Sn

Gas

Takes the shape and the volume of its container, has particles that are widely separated and move independently of one another

Liquid

Takes the shape of the filled portion of its container, has its own volume, has particles that are randomly arranged and free to move about

green chemistry

The development of chemical processes that prevent pollution and reduce the amount of natural resources used to manufacture various consumer, research, and industrial products

boiling point

The temperature at which a liquid changes to a gas

melting point

The temperature at which a solid becomes a liquid

T/F : All samples of a given pure substance of the same composition regardless of their origin

Trie

T/F : an atomic mass unit is defined using the mass of a particular isotope of carbon

True

A substance composed of two or more elements combined in definite proportions is called a ______

compound

the law of ________ predicts that samples of the same compound always contain the same proportion of component elements

definite proportions

Electron

negatively charged particle

Neutron

no charge